In this exercise, using the Henderson-Hasselbach equation, you will be asked to make the necessary computations to prepare a buffer on your own. Choosing from various solutions with corresponding pK, values given on the table below, choose a pair that would be ideal for the preparation of a 100mL buffer solution with a pH of 9.02 a. Selection of the conjugate base pair solutions Using the table of pKa values, pick a pair of solutions appropriate for the preparation of the buffer with the desired pH. Reagent (0.1 M solutions) pka Ammonia 9.25 Acetic acid 4.75 Ammonium Chloride 9.24 Sodium acetate 4.75 Using the equation below, calculate the ratio of [base] to [acid] to get the buffer of desired pH. pH = pK, + log [base[acid] b. Chosen conjugate acid base pair: volume of 0.1 M acid needed: volume of 0.1 M base needed:

In this exercise, using the Henderson-Hasselbach equation, you will be asked to make the necessary computations to prepare a buffer on your own. Choosing from various solutions with corresponding pK, values given on the table below, choose a pair that would be ideal for the preparation of a 100mL buffer solution with a pH of 9.02 a. Selection of the conjugate base pair solutions Using the table of pKa values, pick a pair of solutions appropriate for the preparation of the buffer with the desired pH. Reagent (0.1 M solutions) pka Ammonia 9.25 Acetic acid 4.75 Ammonium Chloride 9.24 Sodium acetate 4.75 Using the equation below, calculate the ratio of [base] to [acid] to get the buffer of desired pH. pH = pK, + log [base[acid] b. Chosen conjugate acid base pair: volume of 0.1 M acid needed: volume of 0.1 M base needed:

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A student needs to prepare a buffer solution with a pH of 6.00. Assuming a pKą of 4.86, how many mL of 0.1 M B¯ would need to be added to 17.0 mL of 0.1 M HB prepare this buffer? Please include a proper (abbreviated) unit. HINT: Use pH = pKa + log ([B minus]/[HB]) or, if concentrations are the same, pH = pka + log (Volume of B minus/ Volume of HB) Your Answer: Answer units
A buffer solution is prepared which is 0.140 M both in lactic acid (CH3CHOHCO₂H) and in sodium lactate (CH3CHOHCO₂Na). 1.38×10-4 for lactic acid. Ka What is the pH of this solution? = 3.860 You are correct. Your receipt no. is 153-562 When 1.94 mL of 0.120 M HCI is added to 11.0 mL of this buffer solution, what is resulting change in pH? 0.11 Previous Tries Submit Answer Incorrect. Tries 33/99 Previous Tries This discussion is closed.
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Determine the [H3O+H3O+] of the eight buffer solutions made by mixing 1.10 M acetic acid and 0.900 M sodium acetate solutions according to the following volumes. The pKa for acetic acid, CH3CO2HCH3CO2H (HAc), is 4.745. You will also need this information in your post-lab. It is highly suggested you write these calculations down (both unrounded and rounded values) to use later. Solution 1.10 M Acetic Acid (mL) 0.900 M Sodium acetate (mL) [H3O+H3O+] (M) 1 8.00 2.00 Solution 1 Concentration 2 7.00 3.00 Solution 2 Concentration 3 6.00 4.00 Solution 3 Concentration 4 5.00 5.00 Solution 4 Concentration 5 4.00 6.00 Solution 5 Concentration 6 3.00 7.00 Solution 6 Concentration 7 2.00 8.00 Solution 7 Concentration 8 1.00 9.00 Solution 8 Concentration Solution 1 Concentration: M Solution 2 Concentration: M Solution 3 Concentration: M Solution 4 Concentration: M…
(using henderson hassel bach equation) Describe in detail how you would make 500mL of a 250mM buffer at pH 9.0 from the following list of chemicals: 1M NaOH. 1M HCl. Ammonium chloride salt (solid). 30% Ammonia (liquid). For your buffer preparation give all species present and their concentrations in solution. first use henderson hasselbach equation to find the relation between weak electrolyte and its conjugate ion.The buffer concentration is 250 mM. This means that the total concentration of the weak electrolyte and its conjugate base is 100 mM. use this relation to get the concentration of both and then using that concentration or molarity and volume which is 500ml and molar mass find the mass of weak electrolyte and its conjugate base.
Phosphoric acid is a triprotic acid (Kal = 6.9 x 10-3, Ka2 = 6.2 × 10-8, and Ka3 = 4.8 × 10-13). To find the pH of a buffer composed of H, PO, (aq) and HPO (aq), which pKa value should be used in the Henderson-Hasselbalch equation? O pKal = 2.16 pK22 = 7.21 O pKa3 = 12.32 Calculate the pH of a buffer solution obtained by dissolving 10.0 g of KH, PO,(s) and 25.0 g of Na, HPO,(s) in water and then diluting to 1.00 L. pH = II
What is the highest pH that could be used as an effective buffer with B (a generic base) with Kp = (6.46x10^-10) and its chloride salt, HBCI? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible.
Please provide detailed solution and give the explanation of the concept..... A 1.42 L buffer solution consists of 0.176 M butanoic acid and 0.280 M sodium butanoate. Calculate the pH of the solution following the addition of 0.077 moles of NaOH. Assume that any contribution of the NaOH to the volume of the solution is negligible. The Ka of butanoic acid is 1.52 × 10-5. Note: The buffer solution consists of the weak acid butanoic acid, C3H7COOH, and its conjugate base butanoate, C3H7COO–. The added NaOH, a strong base, will react with a stoichiometrically equivalent amount of butanoic acid to produce butanoate. Start by determining the initial amount, in moles, of butanoic acid and butanoate in the buffer solution before the addition of NaOH.
Phosphoric acid is a triprotic acid with the pKa values pKal = 2.148, pKa2 = 7.198, and pKa3 = 12.375. You wish to prepare 1.000 L of a 0.0200 M phosphate buffer at pH 7.560. To do this, you choose to mix the two salt forms involved in the second ionization, NaH, PO, and Na, HPO,, in a 1.000 L volumetric flask and add water to the mark. What mass of each salt will you add to the mixture? mass NaH, PO4 g mass Na, HPO, = g What other combination of phosphoric acid and its salts could be mixed to prepare this buffer?
Calculate the pH of 1.00 L of the buffer Part 1 of 3 Note: Reference the pK of acids at 25 °C table for additional information. a 4.73 pH of starting buffer: Be sure your answer has the correct number of significant digits. Part 2 of 3 ×... 4.76 Part 3 of 3 x10 × pH after addition of 0.040 mol NaOH: Be sure your answer has the correct number of significant digits. 4.61 x10 X Ś x10 0.99 M CH3COONa 1.02 M CH₂COOH X before and after the addition of the following species. (Assume there is no change in volume.) Ś pH after further addition of 0.133 mol HCl: Be sure your answer has the correct number of significant digits. Ś
A 1.43 L buffer solution consists of 0.103 M butanoic acid and 0.300 M sodium butanoate. Calculate the pH of the solution following the addition of 0.069 moles of NaOH. Assume that any contribution of the NaOH to the volume of the solution is negligible. The K, of butanoic acid is 1.52 x 10-5. pH =