Determine the pH of a buffer that is 0.95 M HBRO and 0.68 M KBRO. The value of pKa for HBRO is8.68.13NEXTBased on the given yalues, set up ICE table in order to determine the unknown.HBRO(aq)H,O(1)H̟Oʻ(aq)BrO(aq)Initial (M)0.95Change (M)Equilibrium (M)5 RESET0.950.688.68+x+2x0.95 + x0.95 - x0.95 + 2x0.95- 2x0.68 + x0.68 - x0.68 +2x-2x0.68-2x

Given data is as follows: The concentration of HBrO = 0.95 M The concentration of kBrO = 0.68 M The…

Answered: Determine the pH of a buffer that is…

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter25: Ph Measurements-buffers And Their Properties

Section: Chapter Questions

Problem 5ASA

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Marble is almost pure CaCO3. Acid rain has a devastating effect on marble statuary left outdoors. Assume that the reaction which occurs is CoCO3(s)+ H+(aq)Ca2+(aq)+HCO3(aq) Neglecting all other competing equilibria and using Tables 15.1 and 13.2, calculate (a) K for the reaction. (b) the molar solubility of CaCO3 in pure water. (c) the molar solubility of CaCO3 in acid rainwater with a pH of 4.00.
A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of the titration.
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
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A buffer is made with 0.50 M weak acid and 0.50 M sodium salt of the conjugate base. The pKa of the weak acid is 9.30 After the addition of a small amount of strong concentrated acid, the new equilibrium concentrations are 0.6 M weak acid and 0.4 M base. Calculate the new pH. Enter result with 2 decimal places, digits only.
A buffer solution is made such that the initial concentrations of lactic acid (HC3H5O3) and the lactate ion (C3HO-) are 0.600 M and 0.620 M, respectively. What is the resulting pH if 300.0 mL of 0.100 M potassium hydroxide is added to 0.600 L of the buffer solution? (The Ka of HC3H5O3 is 1.4 x 10-4.) Answer not in scientific notation
In the titration of a weak acid vsstrong base, 50.00mL base was required to reach equivalence point. When exactly 25.00 mL of base is added, the pH in the solution is found to be 5.28. What is the K of the weak acid?
The electronic meters used to measure pH are calibrated using standard buffer solutions of known pH. For example, the directions for preparing a certain buffer at 25°C are as follows. Dissolve 3.40 grams of KH2PO4(s) and 3.55 grams of Na2HPO4(s) in sufficient water to make 1.00 L of solution. What pH do you calculate for this buffer solution? Please answer very soon will give rating surely
How many moles of CH₃NH₃Cl need to be added to 200.0 mL of a 0.500 M solution of CH₃NH₂ (Kb for CH₃NH₂ is 4.4 × 10⁻⁴) to make a buffer with a pH of 10.90? Let x represent the original concentration of CH3COO- in the water. Based on the given values, set up the ICE table in order to dtermine the unknown.
Q- n A 29.2 mL sample of 0.213 M ethylamine, C2H5NH2, is titrated with 0.273 M perchloric acid. At the titration midpoint, the pH is. Use the Tables link in the References for any equilibrium constants that are required.
A buffer is composed of 0.200 M (CH3)2NH (Kb = 5.9 × 10–4) and 0.250 M (CH3)2NH2NO3. What is the pH of the resulting solution after 0.0750 mol of HCl are added to 250. mL of the buffer? Assume that the change in volume is negligible. Enter your response in pH units to the nearest 0.1.
A buffer is composed of 0.200 M HC2H3O2 (Ka = 1.8 × 10–5) and 0.250 M NaC2H3O2. What is the pH of the resulting solution after 0.0200 mol of KOH are added to 500.0 mL of the buffer? Assume that the change in volume is negligible. Enter your response in pH units to the nearest 0.01.

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