A solution is prepared that is initially 0.15M in methylamine (CH3NH2), a weak base, and 0.44M in methylammonium bromide(CH3NH3Br). Complete the reaction table below, so that you could use it to calculate the pH of this solution.Use x to stand for the unknown change in [OH]. You can leave out the M symbol for molarity.[CHÍNH,] [CH,NH][OH]initial☐☐☐change☐☐final

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Answered: A solution is prepared that is…

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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How to calculate the ph? What would be the result if the acid was a di or tripotic? How do the calculation for them?
Calculate [OH-] and pH for each of the following strongbase solutions: (a) 0.182 M KOH, (b) 3.165 g of KOH in 500.0mL of solution, (c) 10.0 mL of 0.0105 M Ca(OH)2 diluted to500.0 mL, (d) a solution formed by mixing 20.0 mL of 0.015M Ba(OH)2 with 40.0 mL of 8.2x 10-3 M NaOH.
A chemist makes a 1.0 L of a solution that is both 0.6 M NH, and 0.8 M NH,CI. pK, of NH3 = 4.75. What is the pH of this solution? Round your answer to two decimal places. pH =
A solution is prepared at 25 °C that is initially 0.46M in methylamine (CH,NH,), a weak base with K,=4.4 × 10 -4 and 0.28M in methylammonium bromide (CH,NH,Br). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = ||
Chloroacetic acid, HC,H, C10,, has a greater acid strength than acetic acid because the electronegative chlorine atom pulls electrons away from the O-H bond and thus weakens it. Calculate the hydronium ion concentration and the pH of a 3.00 x 10-8 M solution of chloroacetic acid. K, is 1.3 x 10-. [HsO*]=| M pH =
A solution is found to contain 1 x 10-2 OH− ions, determine the pH of this solution.
Phosphoric acid, H, PO, (aq), is a triprotic acid, meaning that one molecule of the acid has pKal pKa2 pKa3 three acidic protons. Estimate the pH and the concentrations of all species in a 0.250 M phosphoric acid solution. 2.16 7.21 12.32 [H, PO,] = M [H*] = M [H,PO,] = M [OH¯] = M * TOOLS x10 [HPO;" ] = 6.2 х10-8 1.34 M pH = [PO] = M
C3H,NH, COOH, para-aminobenzoic acid (PABA), is used in some sunscreen agents. Calculate the concentrations of hydronium ion and para-aminobenzoate ion, C;H,NH,C00", in a 5.0 x 10-2 M solution of the acid. The value of K, is 2.2 x 10-. Concentration of hydronium ion = M Concentration of para-aminobenzoate ion = M
If 20 ml of 0.1M NH4OH is added to 10 ml of 0.2M NH4Cl. What are the equilibrium concentrations of all ions and the pH of the resulting solution, given that the equilibrium constant is 1.8x10^-5
A solution of phenol (HC₆H₅O) is prepared by dissolving 0.385 g of phenol in 2.00 L of H₂O. The solution has a pH = 6.29. Determine the value of Ka for phenol. Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. Based on your ICE table and definition of Ka, set up the expression for Ka and then evaluate it. Do not combine or simplify terms.
A solution is prepared that is initially 0.38M in ethylamine (C₂H5NH₂), a weak base, and 0.12M in ethylammonium chloride (C₂H5NH₂C1). Complete the reaction table below, so that you could use it to calculate the pH of this solution. Use x to stand for the unknown change in [OH-]. You can leave out the M symbol for molarity. initial change final [C,HẠNH,] 0 0 [C,HẠNH] 0 0 [OH-] 0 010 X Ś
0.185 M in HCHO2 (Ka = 1.8 ×x 10-4) and 0.230 M in HC2H3O2 (Ka = 1.8 × 10-5) Express your answer to two decimal places. ? Find the pH of each mixture of acids. pH = 2.11 Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining In a mixture of two acids that have similar K, values, the dissociation of one acid affects the dissociation of the other acid, and vice versa. Prepare two ICE tables (where I means initial, C means change, and E means equilibrium), one for the dissociation of HCHO2 and one for the dissociation of HC2H3O2. Use the given acid-dissociation constants to calculate the amount of H3O+ produced by each acid in the pair. Part D 6.00x10-2 M in acetic acid (Ka = 1.8 × 10-5) and 6.00×102 M in hydrocyanic acid (Ka = 4.9 × 10-10) Express your answer to two decimal places. ? pH =

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