Please use pictures as reference. Use part A information to find part B answer.Question: How does this compare to the solubility of Mg(OH)2 in pure water? Find Part B answer Then convert the molar solubility to g per 100Part BHow does this compare to the solubility of Mg(OH)2 in pure water?Express your answer as a ratio to two significant figures.View Available Hint(s)V7 ΑΣΦ-1.63.106SubmitPrevious Answers$₁X Incorrect; Try Again; 5 attempts remainingMacBook Air100 px2.1x10 mol Mg(OH),1X1.2 x 10-8 g Mg(OH)2/100 mL?1X1000 LXX58.33 g Mg1 mol Met ▼Part ACalculate the solubility (in grams per 1.00 x 10² mL of solution) of magnesium hydroxide in a solution buffered at pH = 12.Express your answer to two significant figures.▸ View Available Hint(s)S1 = 1.2x10-8 g/ (1.00 x 10² mL)SubmitPrevious Answers✓ CorrectBegin by writing the reaction by which solid Mg(OH)2 dissolves into its constituent aqueous ions:Mg(OH)2 (s) = Mg²+ (aq) + 2OH(aq)Write the equilibrium expression for KKsp = [Mg2+][OH-]²The solubility of Mg(OH)2 depends on the concentration of OH ions. The calculation of the OH ion concentration is summarized in the hint for this part([OH] = 1.0 x 10-2 M). In a buffered solution, [OH-] remains constant and, therefore, the molar solubility of Mg(OH)2 equals [Mg²+]:S₁ =Then convert the molar solubility to g per 100 mL:Part BS₁ = 100 x=How does this compare to the solubility of Mg(OH)2 in pure water?Express your answer as a ratio to two significant figures.=[Mg²+]KJOH1X1000 pa1.2 x 10-8 g Mg(OH)2/100 mLX2.06x10-13(1.0x10-2)22.1 x 10 9 M.2.1x10 mol Mg(OH)1XX58.33 g Mg(OH)₂Imol Mg(OH),

Answered: Image /qna-images/answer/a9fa3d76-42e4-4f45-b8f4-3d24d2e8ab36.jpg

T Part B How does this compare to the solubility of Mg(OH)2 in pure water? Express your answer as a ratio to two significant figures. View Available Hint(s) |2| ΑΣΦΑ -6 $1.63 107 Submit Previous Answers ?

T Part B How does this compare to the solubility of Mg(OH)2 in pure water? Express your answer as a ratio to two significant figures. View Available Hint(s) |2| ΑΣΦΑ -6 $1.63 107 Submit Previous Answers ?

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 2ALQ

See similar textbooks

Similar questions

What mass of NH4Cl must be added to 0.750 L of a 0.100-M solution of NH3 to give a buffer solution with a pH of 9.26? (Him: Assume a negligible change in volume as the solid is added.)
Ammonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a buffer with a pH of 9.56, 15.0 g of NH4Cl are added. How many liters of NH3; at 25C and 0.981 atm should be used to prepare the buffer? Assume no volume changes and ignore the vapor pressure of water.
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
A sodium hydrogen carbonate-sodium carbonate buffer is to be prepared with a pH of 9.40. (a) What must the [ HCO3 ]/[ CO32 ]ratio be? (b) How many moles of sodium hydrogen carbonate must be added to a liter of 0.225 M Na2CO3 to give this pH? (c) How many grams of sodium carbonate must be added to 475 mL of 0.336 M NaHCO3 to give this pH? (Assume no volume change.) (d) What volume of 0.200 M NaHCO3 must be added to 735 mL of a 0.139 M solution of Na2CO3 to give this pH? (Assume that volumes are additive.)
When a diprotic acid. H2A. is titrated with NaOH, the protons on the diprotic acid are generally removed one at a time, resulting in a pH curve that has the following generic shape: a. Notice that the plot has essentially two titration curves. If the first equivalence point occurs at 100.0 mL NaOH added, what volume of NaOH added corresponds to the second equivalence point? b. For the following volumes of NaOH added, list the major species present after the OH reacts completely. i. 0 mL NaOH added ii. between 0 and 100.0 mL NaOH added iii. 100.0 mL NaOH added iv. between 100.0 and 200.0 mL NaOH added v. 200.0 mL NaOH added vi. after 200.0 mL NaOH added c. If die pH at 50.0 mL NaOH added is 4.0 and the pH at 150.0 mL NaOH added is 8.0, determine the values Ka and Ka. for the diprotic acid. d.
2. If an acetic acid/sodium acetate buffer solution is prepared from 100. mL of 0.10 M acetic acid what volume of 0.10 M sodium acetate must be added to have a pH of 4.00? 100. mL 50. mL 36 mL 18 mL
Sketch two pH curves, one for the titration of a weak acid with a strong base and one for a strong acid with a strong base. How are they similar? How are they different? Account for the similarities and the differences.
How much solid NaCH3CO23H2O must be added to 0300 L of a 0.50-M acetic acid solution to give a buffer with a pH of 5.00? (Him: Assume a negligible change in volume as the solid is added.)
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
Mixing together solutions of acetic acid and sodium hydroxide can make a buffered solution. Explain. How does the amount of each solution added change the effectiveness of the buffer?
A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of the titration.
A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If you wanted to buffer a solution at pH = 4.00 or pH = 10.00, how would you decide which weak acidconjugate base or weak baseconjugate acid pair to use? The second characteristic of a good buffer is good buffering capacity. What is the capacity of a buffer? How do the following buffers differ in capacity? How do they differ in pH? 0.01 M acetic acid/0.01 M sodium acetate 0.1 M acetic acid/0.1 M sodium acetate 1.0 M acetic acid/1.0 M sodium acetate