Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Lactic acid, CH3CH(OH)COOH, has one acidic hydrogen. If a 0.114 M solution of lactic acid has a pH of 2.54, calculate the Ka of lactic acid.
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- Phosphoric acid, H3PO4(aq), is a triprotic acid, meaning that one molecule of the acid has three acidic protons. Estimate the pH and the concentrations of all species in a 0.400 M phosphoric acid solution. pKa1 pKa2 pKa3 2.16 7.21 12.32 [H3PO4]= M [H+]= M [H2PO4−]= M [OH−]= M [HPO2−4]= M pH= [PO3−4]= Marrow_forwardCalculate K₂ or K from experimental data. The pH of a 0.14-M solution of chlorous acid (HCIO₂) is measured to be 1.49. Use this information to determine a value of Ka for chlorous acid. HCIO₂(aq) + H₂O(l)=CIO₂ (aq) + H₂O˚(aq) K₂ =arrow_forwardThe acidity of a solution is measured by its pH. If Ht represents the concentration of hydrogen ions (in moles/liter) in the solution, the pH is defined by pH - log Ht| Based on careful measurements and calculations, a chemist examines two solutions and asserts: "The hydrogen ion concentration of Solution A is 65.86% greater than the hydrogen ion concentration of Solution B." If the pH of solution B is 10.00, determine the pH of Solution A. Report your answer to two decimal places. Solution A has pH equal to Number (Report to the nearest 0.01)arrow_forward
- The pH of a 0.224 M solution of a weak acid, НВ, is 2.63. What is Ka for the weak acid?arrow_forwardFor each of the following entities • Identify it as a strong or weak acid. • Select the correct arrow to show the changes that occur when the acids are placed in water. • Select the approximate pH for each resulting solution. HCI(aq) is classified as a + acid. The reaction equation with water utilizes which of the following arrows? Choice A Choice B 7 >>7 H2SO3(aq) is classified as a The reaction equation with water would utilize which of the following arrows? Choice A Choice B < 50% H2SO3(aq) + H20(I) • HSO3 (aq) + H30*(aq) The approximate pH of the solution would bearrow_forwardHX is a weak acid: Ka = 5.52 × 10–7. Calculate the pH of a solution in which [HX] = 0.0501 M and [X1–] = 0.00845 M.arrow_forward
- (a) Using the expression Ka=[H+][A−]/[HA], explain how to determine which solution has the lower pH, 0.10MHF(aq) or 0.10MHC2H3O2(aq). Do not perform any numerical calculations. (b) Which solution has a higher percent ionization of the acid, a 0.10M solution of HC2H3O2(aq) or a 0.010M solution of HC2H3O2(aq) ? Justify your answer including the calculation of percent ionization for each solution.arrow_forwardA 0.018 M solution of salicylic acid, HOC6H4CO2H, has the same pH as 0.0038 M HNO3solution. (a) Write an equation for the ionization of salicylic acid in aqueous solution. (Assume only the –CO2H portion of the molecule ionizes.) (b) What is the pH of solution containing 0.018 M salicylic acid? (c) Calculate the Ka of salicylic acid.arrow_forwardDetermine the pH of a 0.10 M solution of sodium acetate (CH3COONa) at 25°C. (Ka of acetic acid = 1.8 ×10−5.) pH =arrow_forward
- The pH of an aqueous solution of 0.400 M hydrocyanic acid, (Ka (HCN) = 4.00 × 10-10) isarrow_forwardFind the pH of the following solutions: 0.03M trichloroacetic acid, Cl3CCO2H, pKa = 0.638arrow_forwardIf 7.1 g of butanoic acid, C₂H₂ O₂, is dissolved in enough water to make 1.0 L of solution, what is the resulting pH? Look up the K₁ value in the Table of Ionization Constants. pH =arrow_forward
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