
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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The Ka for formic acid (HCO2H) is 1.8x10-4, What is the pH of a 0.20M aqueous solution of sodium formate (NaHCO2)?
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- Phosphoric acid, H₂PO4(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 0.500 M phosphoric acid solution. [H₂PO₂] = [H₂PO] = [HPO²] = [PO³] = M M M M pKal 2.16 [H+] = [OH-] = pH = pK₂2 7.21 pK₂3 12.32 M Marrow_forwardSuppose that 80.0 mL of an aqueous 0.200 M methylamine, CH3NH2(aq), is titrated with a 0.400 M HCl(aq) solution. Calculate the pH at 10.0 mL intervals of added HCl(aq), up to 50.0 mL, and plot the titration curve. Assume that the volumes are additive. Use pKb = 3.34 for methylamine.arrow_forwardCalculate pH and pOH for each of the following solutions and determine whether thesolution is acidic, basic or neutral:(i) [H3O+] = 4.1 x 10-10 M (ii) [OH–] = 7.6 x 10-3 M(iii) [OH–] = 6.9 x 10-4 M (iv) [H3O+] = 3.5 x 10-6 Marrow_forward
- The pH of a 0.16 M solution of a weak acid, HA, is 2.85. What is the value of Ka for the weak acid?arrow_forwardThe ka of an unknown acid, HYO₂, is determined to be 5 x 10⁻² empirically. What is the pH of a 0.1 M solution of HYO₂?arrow_forwardThe pH of an aqueous solution of 0.506 M benzoic acid , C6H5COOH isarrow_forward
- The pH of an aqueous solution of 0.149 M potassium acetate, (Assume that KCH3COO, is K. (HCH3COO) = 1.80 × 10-5.) This solution isarrow_forwardOver the past 250 years, the average upper-ocean pH near the Pacific Northwest has decreased by about 0.1 units, from about 8.2 to 8.1. This drop in pH corresponds to an increase in acidity of about 30%. When CO2 levels in seawater rise, the availability of carbonate ion, CO32−, makes it more difficult for marine organisms to build and maintain shells and other body parts from calcium carbonate. Calculate H3O+ and OH− concentrations at pH levels of 8.2 and 8.1. Demonstrate by calculations that this decrease in pH corresponds to an increase in acidity of about 30%. Explain the relationship between the pH of seawater and the availability of carbonate ions. Does the change in pH from 8.2 to 8.1 result in an increase or decrease in the availability of carbonate ions?arrow_forwardCalculate the pH of a weak base solution ([B] > 100 K₂). Calculate the pH of a 0.247 M aqueous solution of hydroxylamine (NH₂OH, K₂ = 9.1×109) and the equilibrium concentrations of the weak base and its conjugate acid. pH [NH₂OH] equilibrium (NH3OH*]equilibrium ΣΣarrow_forward
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