Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Calculate the pH of a 0.10-M solution of aluminum chloride, which dissolves completely to give the hydrated aluminumion [Al(H2 O)6]3+ in solution.
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- Given the pKa of hypochlorous acid, HOCl, is 7.54. What is the pH of a solution which consists of 0.20 M HOCl and 0.70 M OCl-?arrow_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_forwardWrite a balanced equation for the dissociation into ions of each of the following soluble salts in aqueous solution. (Use the lowest possible coefficients. Omit states of matter.) RbNO3 Al2(SO4)3arrow_forward
- 5 A chemistry graduate student is given 450. mL of a 0.10M ammonia (NH3) solution. Ammonia is a weak base with K, = 1.8 × 10. What mass of NH4Cl should the student dissolve in the NH3 solution to turn it into a buffer with pH = 9.11? You may assume that the volume of the solution doesn't change when the NH4Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. ☐ ☐ x10arrow_forwardwrite the formula for the salt formed by mixing Pb2+(aq) and OH- ions as PbOH or PbOH2. Explain why the correct formula is Pb(OH)2, and sketch a molecule (or formula unit) of this substance, clearly indicating the charge on each contributing ion or complex ion.arrow_forwardCalculate the pH and pOH for the solution with [Ca(OH)2] = 4.29 x 10–5 M. Is the solution acidic or basic?arrow_forward
- What is the molar hydronium ion concentration in solutions with each of the following pH values? (a) 1.0 [H3O+] = M (b) 5.0 [H3O+] = M (c) 9.0 [H3O+] = M (d) 12.0 [H3O+] = Marrow_forwardA student prepares a solution for titration by adding a 10.00 mL aliquot of a solution saturated with Ca(OH)2 at 82.9°C to 25.0 mL of deionized water. This solution is titrated with a standardized 0.01252 M HCl solution. The equivalence point is observed after 17.94 mL of the HCl solution has been added. Use this data to answer the questions below. Calculate the moles of OH- in the 10.00ml sample. (Hint, moles of OH- at the equivalence point = moles HCl) Your answer should have 4 sig figs. Enter answers in scientific notationarrow_forwardCalculate the pH of a 0.383 M NH, solution. NH, has a Kp 1.8 × 10-5. 3 pH =arrow_forward
- What is the pH of a 0.950 M solution of Na2HPO4?arrow_forwardA chemistry graduate student is given 125.mL of a 0.40M ammonia NH3 solution. Ammonia is a weak base with Kb = 1.8x10−5. What mass of NH4Cl should the student dissolve in the NH3 solution to turn it into a buffer with pH = 9.03? You may assume that the volume of the solution doesn't change when then NH4Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.arrow_forwardRichard and Jessica are lab partners. They pour 40.0 mL of a 0.200 M HC2H3O2 solution into a 250 mL flask. They then set up a burette and add 0.250 M NaOH solution to the burette. They are asked to fill in the table below. The first box asks for the pH of the acetic acid without any NaOH added. The second through tenth boxes show the pH after the indicated amounts of NaOH are added to the acetic acid solution. Please show your work for the first, sixth and tenth boxes. The initial reaction is: H₂O (L) + HC2H3O2 (aq) = H₂O* (aq) + C₂H₂O₂ with Ka = 1.8 x 105 and the reaction involving NaOH is: NaOH (aq) + HC₂H₂O₂ (aq) = H₂O (L) + C₂H₂O₂ (aq). mL of NaOH added pH Box 1 work 0.00 2.72 4.00 8.00 3.46 3.99 12.00 16.00 4.37 H3O+ HCz HyOz | Hz H3 C2H3O2 20.00 24.00 28.00 32.00 36.00 Initial .200 0 PH= 2.72 change -X X X Equilibrium 200-x 1.8×10-5 = x² X X = 3.6 × 10-6 = √x²= √3.6×10-6 1 .200 Box 6 work Box 10 work [H 301 = 0.00189 pH = 100 [H3O+] =arrow_forward
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