An analytical chemist is titrating 83.1 mL of a 0.2800M solution of piperidine (C5H10NH) with a 0.5900M solution of HIO3. The p K₁ of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 44.5 mL of the HIO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO3 solution added. Round your answer to 2 decimal places. pH = 0 X

An analytical chemist is titrating 83.1 mL of a 0.2800M solution of piperidine (C5H10NH) with a 0.5900M solution of HIO3. The p K₁ of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 44.5 mL of the HIO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO3 solution added. Round your answer to 2 decimal places. pH = 0 X

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...

See similar textbooks

Similar questions

Sodium benzoate, NaC6H5COO, is used as preservatives in vinegar, soy sauce, etc. The pH of a 0.10 M aqueous solution of sodium benzoate is 8.60. What is the pKa of benzoic acid, C6H5COOH? Group of answer choices 4.20 5.40 9.80 16.20
A solid hydroxide, with the formula M(OH)3, is dissolve to make a saturated solution. If the pH of the solution is 9.22, what is the Ksp of the solid? What is the solubility of the solid in g/100mL? assume that the molar mass of M is 379.5 g/mol. (In case it isn't obvious, M is a hypothetical metal)
Calculate the pH in the flask when 50mL of a 0.98 M HI solution have been added to 120. mL of a 0.77 M KOH solution. The K₂ for HI is 2.2×10⁹ and the Kb of KOH is 45.
What is the pH of a solution containing 6.65 g sodium acetate (NaC2H302, 82.03 g/mol) in 100.0 mL of solution? The Ka of acetic acid is 1.8 x 10^-5
chemistry Consider 0.10 M solutions of the following compounds: Sr(OH)2, Ca(OCl)2, FeCl3, Ca(C3H5O3)2, and KNO3. Place these solutions in order of increasing pH. (Use the appropriate <, =, or > symbol to separate substances in the list.)
Phenylacetic acid, HC8H702, is one of the substances that accumulates in the blood of persons with phenylketonuria, an inherited disorder which can cause death. A 0.0850 M solution of this substance has a pH of 2.68. What is the value of Ka for phenylacetic acid given this information.
5. Please help me answer all parts to this chemistry question:
We can observe the common-ion effect in action by comparing how much a pure sample of acid dissociates to how much a sample of an acid dissociates when its conjugate base is in solution. Let's consider the oxoacid HIO, which has a Ka of 2.3×10-11. part 1: Calculate the pH of an aqueous solution of 0.100 M HIO. (Due to the low Ka value, you may apply the 5% approximation to avoid the quadratic equation if you wish.) part 2: Complete the RICE table for the dissociation of 0.100 M HIO in a solution with 0.0150 M IO- by selecting the correct answer from any dropdown boxes available. (Remember that the conjugate bases are typically added in as a soluble salt, such as NaIO, but that the salt dissociates completely and the alkali metal cation is a spectator ion.) part 3: Calculate the pH for the solution made from 0.100 M HIO and 0.0150 M IO- . For this case, you can also make the assumption that x will be negligibly small compared to the starting concentrations of the weak acid and…
Consider that 20.0 mL of 0.10 M HA (an arbitrary weak acid, Ka= 1.5 × 10−6) is titrated with 0.10 M NaOH solution. The ionization of HA in water occurs as the following.HA (aq) + H2O(l) ⇌ A-(aq) + H3O+ (aq)The neutralization reaction between HA and NaOH can be expressed as the following. HA (aq) + NaOH (aq) ® NaA (aq) + H2O (l) Answer the following questions. A) What will be the initial pH of the 0.10 M HA solution?
14. Acetic acid is a weak acid with the formula CH3COOH; the Ka for acetic acid is 1.76 x 10-5 In aqueous solution, acetic acid partially dissociates according to the following reaction: CH3COOH + H2O ⇔ CH3COO- + H3O+ Calculate the pH of the acetic acid solution described below: Volume: 100 mL Concentration: 0.1708 M Since this is a weak acid, you can assume the amount of acid dissociated is << 5% of the total amount of acid present. a 3.26 b 1.77 c 2.76 d 2.00 e 0.77
A 4.50−g quantity of a diprotic acid was dissolved in water and made up to exactly 250 mL. Calculate the molar mass of the acid if 25.0 mL of this solution required 12.0 mL of 1.00 M KOH for neutralization. Assume that both protons of the acid were titrated.
Calculate the pH of a solution that is prepared by mixing 25.0 g HC2H3O2 and 25.0 g NaC2H3O2 in 800.0 mL solution (Ka HC2H3O2 = 1.8 x 10-5)