Calculate the pH of a solution that is prepared by dissolving 0.171 mol of formic acid (HCOOH, K, 1.77x104) and 0.450 mol of hydrocyanic acid (HCN, K₂ -6.17-10-10) in water and diluting to 1.80 L. Also, calculate the equilibrium concentrations of HCOOH, HCOO, HCN, and CN". Do not make an approximation unless the initial acid concentration is greater than 1000 x K. (Hint: The pH will be determined by the stronger acid of this pair.) Submit Answer 5 question attempts remaining pH = [HCOOH) = [HCOO) | [HCN] = (CN) - M M M M

Calculate the pH of a solution that is prepared by dissolving 0.171 mol of formic acid (HCOOH, K, 1.77x104) and 0.450 mol of hydrocyanic acid (HCN, K₂ -6.17-10-10) in water and diluting to 1.80 L. Also, calculate the equilibrium concentrations of HCOOH, HCOO, HCN, and CN". Do not make an approximation unless the initial acid concentration is greater than 1000 x K. (Hint: The pH will be determined by the stronger acid of this pair.) Submit Answer 5 question attempts remaining pH = [HCOOH) = [HCOO) | [HCN] = (CN) - M M M M

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

Consider the following data on some weak acids and weak bases: acid base Ка K, name formula name formula 8- 3.0 × 10 - 8 hypochlorous acid HCIO hydroxylamine HONH, 1.1 × 10 -4 6.8 × 10 ethylamine C2H5NH2 | 6.4 × 10 alo -4 hydrofluoric acid HF Ar Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to thể"s will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 М KСІ choose one v 0.1 M KCIO choose one v 0.1 M HONH3Br choose one v 0.1 M NaF choose one v
number three and four please
A diprotic acid, H, A, has acid dissociation constants of K,j = 1.45 x 10-4 and K2 = 5.12 x 10-". Calculate the pH and molar concentrations of H,A, HA, and A²- at equilibrium for each of the solutions. A 0.184 M solution of H,A. pH = 2.2865 [H,A] = 0.1788 [HA"] = 5.17 xI10-3 [A?-] = M 5.12 x10-11 M A 0.184 M solution of NaHA. pH= [H,A] = M. [HA-] = [A2-] = M M
At a particular temperature, the Ka of benzoic acid (C6H5COOH) is equal to 7.1 x 10-5. What is the pH of a solution prepared by combining 0.479 mol of a the acid with 0.143 mol of C6H5COONa (the sodium salt of the acid) in 4.0 L of water? Report your answer to the hundredths place and do not include units. Report your answer to the hundredths place and do not include units.
There is a triprotic acid with the following Ka values: 7.9 x 10-3, 2.0 x 10-7, 6.2 x 10-8. If I take 100 mL of this acid at a concentration of 0.1432 mol/L and add to it 10, 50 and 150 mL of 0.1320 mol/L NaOH what will the final pH values be?
What is the concentration of H3O+ in a solution that is 0.0600 M Hypochlorous acid (HClO)? What is the pH? To solve this problem: Write the acid dissociation equilibrium for HClO Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, ClO- and HClO at equilibrium, in terms of x. Decide if x can be neglected. You may neglect x if the initial concentration of the HClO is greater than 100 times the Ka. You will need the value of Ka. Look it up on the chart (p 4 of packet) Solve for x Find the pH The pH of a 0.0200 M solution of an unknown acid is 2.56. What is the Ka of this acid? To solve this problem: Write the acid dissociation equilibrium for the generic aicd “HA” Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, A- and HA at equilibrium, in terms of x. What is x? Can you find it…
Choose the correct answer from among the alternatives; To make the sentence true: the pH of a solution of oxalic acid (H2C2O4) with a concentration of 0.150M at 298K is 1.16, so the Ka value for the acid ---------------------- A)10 - 2 x 9.5 B)10 - 12 x 5.9 C) 10-12 x 9.5 D) 2-10 x 5.9
5) and 6)
Please help me
Calculate PH for a 0.25 liter solution containing 3.25 gm of potassium cyanide(KCN) , know that Ka(HCN)= 4.9*10-10.
The first disinfectant used by Joseph Lister was called carbolic acid (C6H5OH). At present, this substance is commonly known as phenol (Ka= 1.0 x 10-10). Calculate for the pH of a 0.25 M solution of phenol and the percent ionization. C6H5OH ↔ C6H5O- + H+ pH 3.5 and 2.0 x 10-3 % ionization pH 5.3 and 2.0 x 10-3 % ionization pH 3.5 and 2.0% ionization pH 5.3 and 2.0% ionization
We want to prepare a buffered solution having a pH of 4.97 using concentrated (23.6 M) formic acid (HCOOH) and solid sodium formate (HCOONA). Ką for formic acid is 1.8 x 10-4. Incorrect. Calculate the ratio [HCOO (aq)] / [HCOOH(aq)] in the buffered solution required to achieve a pH of 4.97. [HCOO (aq)] /[HCOOH(aq)] = i 1.68E1 eTextbook and Media Hint Save for Later Attempts: 2 of 3 used Submit Answer