-1Determine the [CO32] in the Na2CO3 solution which you prepared and determinethe expected pH of that solution. Ka for HCO3 = 7.0 x 10-11 M. Compare thecalculated and observed values and comment on the agreement. Data Table II: HydrolysisRecord the actual mass of each of the following solutes:1-159Ammonium chloride, NH4Cl1-1.59Sodium carbonate, Na2CO3Zinc nitrate, Zn(NO3)2. 6H2OAluminum nitrate, Al(NO3)3. 9H₂OSodium sulfite, Na2SO31-1.521.2991.10 g(skip)(skip)1.43 99.Record the pH of the above solutions and the prepared ammonium acetate and sodium hydrogenphosphate solutions to the nearest 0.01 pH units:pH of Ammonium chloride, NH4Cl solutionSodium carbonate, Na2CO3Zinc nitrate, Zn(NO3)2. 6H2OAluminum nitrate, Al(NO3)3. 9H₂OSodium sulfite, Na2SO3pH of Ammonium acetate solutionpH of sodium hydrogen phosphate solution7.10 PH12.110 раPH(skip)(skip)9.00 PH5.16 PH(skip)

Step 1: Step 2: Step 3: Step 4:

Answered: -1 Determine the [CO32] in the Na2CO3…

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 8ALQ: You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major...

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You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
The pH of a 0.20-M solution of HP is 1.92. Determine Ka far HF from these data.
Weak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/A
Define or illustrate the meaning of the following terms: a. amphoteric b. Kw reaction c. Kw equilibrium constant d. pH e. pOH f. pKw Give the conditions for a neutral aqueous solution at 25C, in terms of [H+], pH, and the relationship between [H+] and [OH]. Do the same for an acidic solution and for a basic solution. As a solution becomes more acidic, what happens to pH, pOH, [H+], and [OH]? As a solution becomes more basic, what happens to pH, pOH, [H+], and [OH]?
Isocyanic acid (HNCO) can be prepared by heating sodium cyanate in the presence of solid oxalic acid according to the equation 2NaOCN(s)+H2C2O4(s)2HNCO(l)+Na2C2O4(s) Upon isolating pure HNCO(l), an aqueous solution of HNCO can be prepared by dissolving the liquid HNCO in water. What is the pH of a l00.-mL solution of HNCO prepared from the reaction of 10.0 g each of NaOCN and H2C2O4, assuming all of the HNCO produced is dissolved in solution? (Ka of HNCO = 1.2 l04.)
Rank the compounds in each of the following groups in order of increasing acidity or basicity, as indicated, and explain the order you assign. (a) acidity: HCI, HBr, HI. (b)basicity: H2O, OH-, H-, CI-. (c) basicity: Mg(OH)2, Si(OH)4, ClO3(OH) (Hint: Formula could also be written as HCIO4). (d) acidity: HF, H2O, NH3, CH4
You have a solution of the weak acid HA and add some HCl to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
Write the Lewis structures of the reactants and product of each of the following equations, and identify the Lewis acid and the Lewis base in each: (a) CS2+SHHCS3 (b) BF3+FBF4 (c) I+SnI2SnI3 (d) Al(OH)3+OHAl(OH)4 (e) F+SO3SFO3
Chloroacetic acid, ClCH2CO2H, is a moderately weak acid (Ka=1.40103). If you dissolve 94.5 mg of the acid in water to give 125 ml of solution, what is the pH of the solution?
Estimate the pH of a solution in which crystal violet is yellow and methyl orange is red. (See Fig. 14-8.)
The pH for 0.0850 M solution of C,H,CH,COOH is 2.68. Determine the value of Ka for C,H̟CH,COOH. 1 NEXT Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. C,H,CH,COOH(a q) H,O(1) H,O(aq) CH.CH.COO(aq 1, +6 Initial (M) Change (M) Equilibrium (M)
1. Calculate the H3O+, pH, OH¯, and pOH for a 0.015 M Ca(OH)2 solution. 2. The pH of a 0.02 M solution of a weak acid was measured at 4.6. (a) What is the [H+] in this solution? (b) Calculate the acid dissociation constant Ka and pKa for this acid? 3. Calculate the pH of a 0.010 M hypochlorous acid solution. For HOCI, Ka = 3.5 × 10-8. 4. What is the pH of a 0.19 M monoprotic acid whose Ka is 5.7 x 10-4. 5. The pH of a solution containing 0.010 M lactic acid and 0.087 M lactate is 4.80. Calculate the pKa of the lactic acid.

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