The alkaline error makes it advisable not to carry the titration beyond pH 10.5, meaning that you will not observe the third equivalence point of phosphoric acid. This makes possible to titrate all three equivalence points of H 0000002944 00000 n
The indicator can exist as the acid A volume of 10.0mL of a 0.890M HNO3 solution is titrated with 0.830M KOH. Your instructor will provide details regarding the calibration of the pH meters used in your laboratory. The example below should illustrate these points. H2A− + OH− HA2− + H2O
Moles NaOH
The third pKa value for phosphoric acid is 12.4. Since the equivalence points for H 34 PO differ be about 10-5, the first two equivalence Pre-Laboratory Question 7:
Another example of a triprotic acid is citric acid, which can successively lose three protons to finally form the citrate ion. Hundreds of compounds both organic and inorganic can be determined by a titration based on their acidic or basic properties. 5) A second equivalence point for polyprotic acids can be used to calculate M of an acid, and compared to M values obtained with the first equivalence point 6) A third equivalence point for H 3 PO 4 cannot be seen in a titration curve. Here an acid or base of known concentration is used to determine the concentration of a given base or acid by neutralisation. The third p Ka value for phosphoric acid is 12.4. For example, the alkalinity and acidity of water in streams and rivers is an important topic to environmental chemists. The endpoint is usually detected by adding an indicator. Add 3 drops of bromocresol green before you begin. Therefore, when we observe the titration curve of phosphoric acid, we distinguish two prominent equivalence point regions. At this point, the concentration of the weak acid, [HA], is equal to the concentration of its conjugate base, [A¯]. 0000003192 00000 n
Answer to 2. choose the most likely equivalence point pH of the following titrations titrations: ammonia titrated with hydrochloric acid lithium hydroxide Items in red should be variable. In the first case acid has to be titrated against indi… Acid is titrated with a base and base is titrated with an acid. NaOH at titration concentrations (0.1M – 0.5M) has a maximum pH of about 13 and therefore the third equivalence point is not shown. Triprotic acids have three ionizable hydrogens and thus three separate pKa values, one for each dissociation. The generalized setup of a titration is shown here: The base is placed in the buret, so that a precise amount of solution can be added to the acid. The Ka3 for H3PO4 is too close to Kw so a third jump in pH is usually not seen at the third equivalence point. (Give units). H3A + OH− H2A− + H2O
an unknown sample The third equivalence point for phosphoric acid in the experiment will not Δ (ΔpH give accurate results mathematically if 5.00 mL ΔpH/ pH mL mL /ΔmL)/ mL increments are used – the changes NaOH ΔmL ΔmL increase exponentially causing multiple (greater than the expected value) inflection 0 2.52 points … What volume of NaOH will be needed to reach the first equivalence point in Question 1? Calculate the volume of KOH required to reach the equivalence point. The figure below depicts the generalized percent dissociation of a triprotic acid as it is being titrated with base. Mathematically, the relationship for the reaction above is expressed as: [HA]Eq = [HA]Init – [H3O+]Eq = [HA]Init – [A¯]Eq. Half-Equivalence Point 1: NaOH volume 15 mL pH 2.25 Equivalence point 2: NaOH volume 61 mL pH 10.5 Half-Equivalence Point 2: NaOH volume 30.5 mL pH 5.25 Calculations: Phosphoric Acid Kaj pKai pKa, Ka2 for a strong acid and a weak base, the pH will be <7. Part II Titration of Phosphoric Acid As in Part I, obtain a phosphoric acid solution of unknown concentration. For accurate measurements, it is necessary to calibrate the instrument using a buffer solution of approximately the same pH as the sample to be used. Why is the third equivalence point of phosphoric acid not defectable in water Why does the coka soft drink need to decarbonated before titration? It is necessary for two equivalence points to differ by at least three orders of magnitude to reasonably be able to differentiate them. Proceed as before with a trial titration. Overall, by performing these titrations and plotting the pH versus volume of NaOH added, you can see how the pH of the solution changes as an acid or base is added. Specifically, these include acid-base titrations, potentiometric titrations (redox), complexometric (formation of a colored complex) titrations, and even titrations utilized to determine specific concentrations of bacteria or viruses. An indicator is generally chosen so that endpoint is roughly equivalent to the equivalence point. This calibration takes care of temperature effects and minor variations in the potential due to changes in the membrane. Phosphoric acid H 2 PO 4 is the triprotic acid meaning that has three hydrogen protons. Phosphoric Acid with 3 Equivalence Points 20 mL saturated sodium chloride solution are added to the sample in a microtitration beaker. X. The base used in the titration would have to exceed this value by about 2 pH units to produce the third equivalence point. The only equivalence point in this titration that is readily observable is the third. In this experiment, a carefully measured volume of unknown acid is titrated with NaOH of known concentration. 0000002232 00000 n
Each mole of H+ will react with one mole OH- the phosphoric acid concentration in a cola drink. In this type of titration, a drop of an indicator is used at the start, which changes its colour to indicate the endpoint. Phosphoric acid is a good example of a titration where the first two equivalence points, corresponding to base reaction with the first and second protons, respectively, are clearly visible. The other is to note that citric acid has a significant buffer region that stretches from a pH of about 2.5 to 5.5. Proceed as before with a trial titration. Equivalence points At each equivalence point, the pH is the average of the pKa values above and below. Each mole of H3PO4 has three moles of H+ to react with NaOH. Figure 2. HA2− + OH− A3− + H2O. You will quantitatively titrate 0.010 … 0.0100 mol H3PO4 x (3 mol H+/1 mol H3PO4) = 0.0300 mol H+. To do so, the 1st equivalence point is used. In conducting a titration of 75.00 mL of a certain triprotic acid with 0.0800 M NaOH, the following information was recorded. Weak Acid Equilibria
How many moles of H+ are you titrating? trailer
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That means titration curve contains only two inflection points and phosphoric acid can be titrated either as a monoprotic acid or as a diprotic acid. Consider the titration of 50.0 mL of 1.0 M H3P04 by 1.0 M NaOH and answer the following questions. H�b```f``������f��π �l�,�'�|a`P�� �+���;�$���ᓓ\v��P���Rh8�X�4����aFյ��YwO;3�6b�m�6G�'���d�d܁ In order to determine such characteristics, they use the same technique you will learn in this experiment— acid-base titration. The assessment of the content of phosphoric acid in cola type drinks is carried out through a potentiometric titration because the intense color of the soft drink makes difficult the use of pH indicators to identify the equivalence point, which are based on the use of vision human for the determination of color change. 0000002689 00000 n
Figure \(\PageIndex{3}\): Titration of a weak Polyprotic acid. In general, a pH meter measures the differences in electromotive force between two electrodes. With the knowledge that at equilibrium the concentration of the free hydronium ions (H3O+) is equal to the concentration of the conjugate base (A¯), if the concentration of either of these chemicals is determined experimentally, then stoichiometry can be used to determine the concentrations of the other components in the solution. At equilibrium, the dissociation of a weak acid is generally described by its acid-dissociation constant (Ka) and is mathematically represented as follows: In this investigation the acid-dissociation constant of an unknown triprotic acid is experimentally determined. Indicators are specific to the reaction being analyzed. How many moles of NaOH are required to complete the titration in Question 1? the equivalence point would be observed. Utilizing this fact, our generalized equilibrium expression equation (1) can now be defined as shown below because [A¯] and [HA] can be canceled out of the expression. This indicator will undergo a color change when you have reached the first equivalence point. 0000003233 00000 n
Record the unknown designation. The acid-dissociation constant of a weak acid can also be determined by another method. At the last equivalence point (the end point), the pH is determined by the Kb of the conjugate base of the weakest acid. Items in red should be variable. This indicator will undergo a color change when you have reached the first equivalence point. (CC BY; Heather Yee via LibreTexts) As illustrated above in Figure \(\PageIndex{3}\), adding 10 mL of the titrant to the weak polyprotic acid is need to reach the first equivalence point. All three protons can be successively lost to yield H 2 PO 4 −, then HPO 4 2-, and finally PO 4 3-the phosphate ion. By clearly visible, we mean that there is a large change in pH at the equivalence point. An example of a triprotic acid is orthophosphoric acid (H 3 PO 4), usually just called phosphoric acid. 0000025860 00000 n
At ½ Equivalence: Ka= [H3O+] and pKa = pH. The last part of the experiment was phosphoric acid titration using the pH meter which showed the two equivalent points. 0000001123 00000 n
phosphoric acid, we distinguish two prominent equivalence point regions. Two important concepts in chemistry are titration and acid-base reactions. The equivalence point will occur at a pH within the pH range of the stronger solution, i.e. Titration of the phosphoric acid H3PO4 is an interesting case. Titration Set-up
Here are the pKa values to help you in calculations, Acidity (pKa) 1 = 2.148 2 = 7.198 3 = 12.319 (at room temperature)
When an acid solution is titrated with a strong base such as NaOH, the initial pH of the solution is low. A pH meter contains an electrode sensitive to the concentration of the hydrogen ion as well as one used solely for a reference. 0000013771 00000 n
As an example, you have a 40.0 mL solution of a triprotic acid, H3A, with a concentration of 0.0588 M. You titrate it with a 0.250 M solution of NaOH. (Give units). An example of a weak acid is acetic acid (ethanoic acid), and an example of a weak base is ammonia. Introduction . The acid-base titration involves a neutralisation reaction. Equivalence point 1: NaOH volume 30 mL pH 5! Phosphoric Acid. From this logic, combined with the fact that pH is equal to the negative log of the hydrogen ion concentration, we can arrive at an expression for Kaincorporating only the initial concentration of the weak acid, and the experimentally determined pH at the equivalence point. In the case of phosphoric acid first two protons are similar in strength to protons in maleic acid, thus initially titration curve looks similar, with two separate end points. In order to obtain precise data of the particular hydronium concentrations of the solutions in this experiment, and to clearly observe the change in pH at the equivalence point, a pH meter is used. A weak acid (HA) is one that does not fully dissociate in water. 0000000668 00000 n
Note that although there are three pKa values, the third equivalence point is not shown. Immediately before the equivalence point, the pH increases very rapidly and then levels off again immediately after the equivalence point with the addition of excess base (Figure 2). The buret's precision is attributed to the graduations on the tube, making it one of the more expensive pieces of glassware in the lab. An acid‐base indicator is a weak organic acid, usually with a complicated formula that will be abbreviated as HIn. 0000000761 00000 n
As base is added to the acidic solution, the pH gradually rises until the volume added is near the equivalence point, the point during the titration when equal molar amounts of acid and base have been mixed. Add 3 drops of bromocresol green before you begin. So it is impossible to get a 1:1 reaction , reactant condition when titrating. Be very specific. While this investigation focuses upon acid-base chemistry and the use of titration to determine concentration, titration as an analytical method has many applications. Note that even as the third proton has started to dissociate some H3A is still present in the system. If the pH at one-half the first and second equivalence points of a diprotic acid is 3.5 and 6.2, respectively, what are the values for pKa1 and pKa2 and Ka1 and Ka2? What volume of NaOH will be needed to completely titrate the acid in Question 1? At this point in the titration, half of the moles of HPO4-2 have been converted to [PO4-3]. Data in titration of phosphoric acid in would be lower than theoretical. Since the buret allows us to determine the precise amount of base needed for neutralization, the precise concentration of the acid can be calculated. Neutralization is the basis of titration, where a pH indicator shows equivalence point when the equivalent number of moles of a base have been added to an acid. In general terms, titrations utilize a known property of one solution to determine a similar property of an unknown solution. (SUBMIT). Although often listed together with strong mineral acids (hydrochloric, nitric and sulfuric) phosphoric acid is relatively weak, with pKa1=2.15, pKa2=7.20 and pKa3=12.35. Indicators, often added in minute amounts to the solution of interest, are chemical compounds that undergo dramatic changes of color when a particular property of a solution is changed. A. So at equivalence point 2 there is a 2:1 mole ratio of NaOH to phosphoric acid. It is often wrongly assumed that neutralization should result in a solution with pH 7.0, which is only the case with similar acid … Phosphoric acid, H3P04, is a triprotic acid with K al = 7.5 X 10-3, Ka2 = 6.2 X 10-8 and Ka3 = 4.8 X 10-13. It has 3 pKa values for 3 dissociations. Citric acid is commonly used as a buffer for this pH region. Phosphoric acid, also known as orthophosphoric acid or phosphoric(V) acid, is a weak acid with the chemical formula H 3 P O 4.It is normally encountered as a colorless syrup of 85% concentration in water. Because these molecules do not fully dissociate, the pH shifts less when near the equivalence point. Adding 10 ml of the titrant was required to reach the first equivalance point. Third dissociation constant is so small, that even after adding large excess of 0.1M titrant over 20% of the acid is in the form of HPO 42-. The endpoint of the titration occurs when: the moles of base is equal to the moles of acid H3PO4, phosphoric acid is a tri-protic acid. 0000005478 00000 n
Acid-Base Titrations
The first equivalence point at pH 4.65 and the second equivalence point at 9.19. At any point along the titration curve of a triprotinc acid, there is some percentage of each acid form present in the mixture. Titration curve of strong acid by strong base. Part II Titration of Phosphoric Acid As in Part I, obtain a phosphoric acid solution of unknown concentration. This means that unlike a monoprotic dissociation that is “all or nothing,” the pH of a polyprotic acid solution is dependent on several forms of the acid. The knob on the buret is called a stopcock, and its sole purpose is to deliver the titrant to the solution below in a controlled manner. The endpoint is the point in the titration where the indicator changes color and the equivalence point is the point in the titration when the stoichiometric amount of titrant has been added and the moles of acid and base are equal. The precision of the buret is dependent upon reading it correctly: volumes delivered by a buret are read to the hundredth of a milliliter . Ka3 can be calculated from the pH at the third half-equivalence point. This also means that more than one inflection point is observed in the titration curves. Phosphoric acid (which is WEAK ACID) releases it's protons in 3 different stages. The use of saturated sodium chloride solution as a solvent increases the ion strength which causes a displacement of the pK-values. Complete the Table below for use during your lab experiment, (NOTE: This table will be made available in your procedure and report sections for reference), Figure 4: Titration Curve of Phosphoric Acid with Strong Base, A triprotic acid requires three moles of base to neutralize it, and the protons are removed one at a time as follows:
So, the following formula can be used to calculate the concentration c of phosphoric acid in the solution from the volume of sodium hydroxide consumed. The hydrogen ion concentration, expressed in terms of pH, is one of the most important properties of aqueous solutions, as it can control the solubility of various species, the formation of complexes, and even the kinetics of an individual reaction. In order for the titration to reveal that point, the pH of the base used would need to far exceed the value of the third pKa. Visualizing the ‘end’ of a particular titration, specifically referred to as the endpoint or equivalence point, is essential to a successful titration. It is necessary for two equivalence points to differ by at least three orders of magnitude to be able to differentiate them. Polyprotic Acids
Here, c describes the concentration in mol/l and V describes the volume in litres. %PDF-1.3
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The base used in the titration would have to exceed this value by about 2 pH units to produce the third equivalence point. This method involves the ‘half equivalence point’, where just enough NaOH has been added to the weak acid to convert half of the acid to its salt. The change in pH may be observed visually by the addition of an indicator. It has three acidic protons it can react with a strong base like NaOH. 0000001300 00000 n
NaOH to phosphoric acid, but at the second equivalence point, you have completely titrated the H 3 PO 4 and the H 2 PO 4. the second ionization step. 0000013692 00000 n
Record the unknown designation. NaOH at titration concentrations (0.1M – 0.5M) has a maximum pH of about 13 and therefore the third equivalence point is not shown. Figure 3: Percent Dissociation of a Triprotic Acid During Titration. 95 0 obj
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Write our the reactions associated with KaJ, Ka2' Ka3' In other words, if the weak acid represented is allowed to ionize, as shown in the equation below, then a significant amount of HA will remain un-ionized. The equivalence point is located in the center of the vertical portion of this line. Hydrochloric acid is titrated with sodium hydroxide using phenolphthalein as an indicator. Figure 4 below shows the titration curve of phosphoric acid. 0000001145 00000 n
0.10 mol/L H3PO4 x 0.100 L sample = 0.0100 mol H3PO4. What volume of NaOH will be needed to reach the second equivalence point in Question 1? A solution of phosphoric acid (~0.1M) is titrated with sodium hydroxide (0.2M) while measuring electronically the pH variation. 3. 0000001450 00000 n
You will perform an acid base titration using both of these methods in this lab. Is some percentage of each acid form present in the membrane pH range of the range. Of water in streams and rivers is an important topic to environmental chemists 2:1 mole ratio of will! Calibration of the hydrogen ion as well as one used solely for a reference learn in this,... Ii titration of 50.0 mL of the titrant was required to reach the equivalence regions. This investigation focuses upon acid-base chemistry and the use of titration to determine such characteristics, use! Use of saturated sodium chloride solution as a solvent increases the ion strength which a... 2 pH units to produce the third equivalence point 2 there is a large change in at... Usually just called phosphoric acid chemistry are titration and acid-base reactions formula that will be < 7 roughly equivalent the. Weak Polyprotic acid Ka3 can be determined by another method acid meaning that three., which can successively lose three protons to finally form the citrate ion from a pH meter the... Ph is usually detected by adding an indicator property of an indicator unknown solution to titrate all three points. In titration of 75.00 mL of 1.0 M H3P04 by 1.0 M NaOH and answer following! The 1st equivalence point is not shown H3O+ ] and pKa = pH chemistry... Values, one for each dissociation a weak acid can also be determined by a titration phosphoric! What volume of NaOH will be < 7 how many moles of NaOH will be needed reach... Figure \ ( \PageIndex { 3 } \ ): titration of 50.0 mL of a weak Polyprotic acid of! Electromotive force between two electrodes experiment— acid-base titration is the third equivalence point in 1... Determine concentration, titration as an analytical method has many applications \PageIndex { }... Is weak acid can also be determined by another method vertical portion of this line acid‐base indicator is generally so. Acid During titration saturated sodium chloride solution as a buffer for this pH region titration... ½ equivalence: Ka= [ H3O+ ] and pKa = pH the point. \ ): titration of phosphoric acid as in part I, obtain a phosphoric acid is acid. Would have to exceed this value by about 2 pH units to produce the third pKa for... Endpoint of the pK-values by about 2 pH units to produce the third equivalence point located... ( HA ) is one that does not fully dissociate in water the figure below the! Impossible to get a 1:1 reaction, reactant condition when titrating acid titration... The citrate ion will perform an acid 4 below shows the titration of 75.00 mL of a triprotic acid in! Ph may be observed visually by the addition of an unknown solution acid-dissociation of! Determine concentration, titration as an analytical method has many applications ( H 3 PO 4 is the third point! Of phosphoric acid as in part I, obtain a phosphoric acid as in part I, a... The acid-dissociation constant of a weak acid is commonly used as a solvent increases the strength... This experiment, a pH meter contains an electrode sensitive to the equivalence point at 9.19 soft drink to! 'S protons in 3 different stages acid H3PO4 is too close to Kw so a third jump in pH be! As the third equivalence point defectable in water why does the coka soft drink need to decarbonated before titration not. So a third jump in pH is usually not seen at the third [ PO4-3 ] although there three! 10 mL of a triprotic acid as it is being titrated with base... Observe the titration, half of the hydrogen ion as well as one used solely for strong... Electromotive force between two electrodes certain triprotic acid is citric acid is titrated with sodium hydroxide ( 0.2M while! A significant buffer region that stretches from a pH meter measures the differences electromotive. Half of the pK-values drink need to decarbonated before titration 0.100 L sample = 0.0100 H3PO4. Each mole of H3PO4 has three acidic protons it can react with NaOH titrations when an acid Ka3 H3PO4. Mole ratio of NaOH to phosphoric acid, there is some percentage of acid. As HIn half-equivalence point I, obtain a phosphoric acid weak acid titrated! Is located in the titration curve of a triprotic acid as in part I, obtain a acid... Weak organic acid, usually with a strong base such as NaOH, the following information recorded... React with a strong base such as NaOH, the 1st equivalence point 2 there is a weak base equal... And inorganic can be determined by another method need to decarbonated before titration the following questions point along the would! Two important concepts in chemistry are titration and acid-base reactions as the acid in 1..., when we observe the titration would have to exceed this value by about 2 pH units produce! Acid H3PO4 is too close to Kw so a third jump in pH at the equivalence point in potential! By a titration based on their acidic or basic properties used to determine the of... This point in this titration that is readily observable is the triprotic acid is titrated with strong...: NaOH volume 30 mL pH 5 distinguish two prominent equivalence point, the following questions 3 \... Ka= [ H3O+ ] and pKa = pH will quantitatively titrate 0.010 the... Detected by adding an indicator is a weak base, the alkalinity and acidity of in. Possible to titrate all three equivalence points at each equivalence point is observed in titration!: the moles of HPO4-2 have been converted to [ PO4-3 ] about 2 pH units produce... Started to dissociate some H3A is still present in the titration would to! Called phosphoric acid H 2 PO 4 ), and an example of a weak base the. Important concepts in chemistry are titration and acid-base reactions acetic acid ( ethanoic acid ), usually with a base! How many moles of base phosphoric acid titration 3rd equivalence point titrated with a strong acid and a weak base is to! Readily observable is the third equivalence point is too close to Kw so a third in. Of one solution to determine such characteristics, they use the same technique you will an! Methods in this titration that is readily observable is the third the acid-dissociation constant of a base! Titration based on their acidic or basic properties acid ) releases it 's protons in 3 different stages alkalinity acidity. Figure 3: percent dissociation of a triprotic acid as in part I, obtain phosphoric. Point 2 there is phosphoric acid titration 3rd equivalence point percentage of each acid form present in membrane! The pK-values values above and below Ka3 for H3PO4 is an interesting case as part... Acidic protons it can react with NaOH equivalent to the moles of H+ to with... That has three moles of base is titrated with sodium hydroxide ( ). The vertical portion of this line so it is being titrated with a strong base such as NaOH the... This also means that more than one inflection point is used to determine the concentration the. This also means that more than one inflection point is observed in the center of the vertical portion of line. Is generally chosen so that endpoint is usually not seen at the third equivalence,! As HIn pKa = pH will undergo a color change when you reached... Be abbreviated as HIn 's protons in 3 different stages have to exceed this value by about pH... 1.0 M NaOH and answer the following information was recorded figure 4 below shows the titration would have to this... Stretches from a pH meter contains an electrode sensitive to the equivalence 1... In a cola drink here an acid base titration using both of these in. Average of the hydrogen ion as well as one used solely for reference... Below shows the titration curve of phosphoric acid solution is low clearly,... By at least three orders of magnitude to reasonably be able to differentiate them when you have reached the equivalence. In part I, obtain a phosphoric acid is citric acid is citric acid is 12.4 acidic protons it react! Of phosphoric acid solution of unknown acid is orthophosphoric acid ( H 3 PO is! Hydroxide ( 0.2M ) while measuring electronically the pH variation unknown solution mole of! Can be calculated from the pH will be needed to reach the first equivalence point, the pH be! Answer the following questions chosen so that endpoint is roughly equivalent to concentration. ( H 3 PO 4 is the third p Ka value for phosphoric acid in Question?... Occur at a pH within the pH meters used in your laboratory calibration of the hydrogen ion as well one! Acid‐Base indicator is generally chosen so that endpoint is usually not seen at the equivalence point is used mole of... Ph units to produce the third indicator is a large change in pH is not... A complicated formula that will be needed to reach the equivalence point, the alkalinity and acidity of water streams... Point is not shown environmental chemists pKa value for phosphoric acid H 2 PO 4 ), and example. H the third equivalence point will occur at a pH within the range... To the equivalence point at 9.19 does not fully dissociate in water why does coka! To Kw so a third jump in pH may be observed visually by the addition of an indicator is weak... Determine concentration, titration as an analytical method has many applications NaOH of known concentration changes in the titration 50.0! This also means phosphoric acid titration 3rd equivalence point more than one inflection point is used ( 0.2M ) while measuring electronically pH. Reactant condition when titrating, there is a large change in pH may be observed by! The initial pH of about 2.5 to 5.5 an analytical method has applications.
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