Concept explainers
(a)
Interpretation:
A net ionic equation for the reaction of
Concept introduction:
Net ionic equation is the ionic equation in which reactants are written in the form of ions if they occur as ions in a reaction medium and product form are shown as combination of ions. The charges of ions and each atom in the reaction are balanced.
(b)
Interpretation:
A net ionic equation for the reaction with aqueous
Concept introduction:
Net ionic equation is the ionic equation in which reactants are written in the form of ions if they occur as ions in a reaction medium and product form are shown as combination of ions. The charges of ions and each atom in the reaction are balanced.
(c)
Interpretation:
A net ionic equation for the reaction with aqueous
Concept introduction:
Net ionic equation is the ionic equation in which reactants are written in the form of ions if they occur as ions in a reaction medium and product form are shown as combination of ions. The charges of ions and each atom in the reaction are balanced.
Want to see the full answer?
Check out a sample textbook solutionChapter 15 Solutions
Chemistry: Principles and Reactions
- 27) Assuming that no equilibria other than dissolution are involved, calculate the concentrations of ions in a saturated solution of each of the following (see Appendix J for solubility products): (a) AgI (b) Ag2SO4 (c) Mn(OH)2 (d) Sr(OH)2·8H2O (e) the mineral brucite, Mg(OH)2arrow_forwardThe solubility of magnesium hydroxide in pure water is 1.3 x 10–4 mol/L. (a) Calculate the Ksp of Mg(OH)2; (b) What isthe pH of saturated Mg(OH)2solution at 25oC? (c) Calculate the solubility of Mg(OH)2 in a solution buffered at pH 9.0?arrow_forwardWrite a net ionic equation for the reaction between aqueous solutions of(a) sodium acetate (NaC2H3O2) and nitric acid.(b) hydrobromic acid and strontium hydroxide.(c) hypochlorous acid and sodium cyanide.(d) sodium hydroxide and nitrous acid.arrow_forward
- A 250-mL buffer solution contains 0.0510 mole of KH2PO4 and 0.0875 mole of K2HPO4. (a) Calculate the molar concentrations of H2PO4–and HPO42–, respectively, in thesolution. (b) What is the pH of the solution? (H2PO4– has Ka = 6.2 x 10–8) (c) Write a net ionic equation for the buffering reaction against a strong acid by this buffer. (d) If 0.012 mole of hydrochloric acid (HCl) is added to the solution, create a reaction table to show the buffering reaction and calculate the molar concentration of H2PO4–and HPO42–, respectively, in the resulting solution after the buffering reaction. (e) What is the pH of the resulting solution?arrow_forward(ii) 2.50 g of sodium acetate, CH3COONA was dissolved in 150.0 mL of water, H2O. A solution of 0.025 M ethanoic acid, CH3COOH was added into the above salt solution. Calculate the pH of the mixed solution.arrow_forward(a) If the molar solubility of CaF2 at 35 oC is 1.24 x 10-3 mol/L, what is the Ksp at this temperature? (b) It is found that 1.1 x 10-2 g of SrF2 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility product for SrF2? (c) The Ksp of Ba(IO3)2 at 25 oC is 6.0 x 10-10. What is the molar solubility of Ba(IO3)2? (d) Answer this question without using any other resources. In part (a), what would the Ksp value of CaF2 be, if it was measured at 25 oC instead of 35 oC?arrow_forward
- We dissolve 2.77 g of an unknown acid, HA, in enough water to produce 25.0 mL of solution. The pH of this solution of HA(aq) is 1.33. We titrate this solution with a 0.250 M solution of NaOH. It takes 41.8 mL of the NaOH solution to reach the equivalence point. (a) What is the molar mass of HA? (b) What is the pKa value of HA(aq)? (c) What is the pH at the equivalence point? (d) What is the pH one third along the titration when you still have twice as much HA(aq) as A-(aq)?arrow_forwardThe mixture of 100.0 mL of 0.100 M NaOH (aq) and 100.0 mL of 0.300 M CH3COOH (aq) will result in a buffer. (a) Explain why the resulting solution is a buffer. (b) What is the pH of this buffer?arrow_forwardThe thermodynamic solubility product of AGCN is 6.0x10-17. (a) What is [Ag+] in a 0.033 M KNO3 solution? 4.0 7.7e-9 X mol·L-1 (b) What is [Ag+] in a 0.033 M KCN solution? 4.0 1.8e-15 X mol·L-1arrow_forward
- Calculate the molar concentration of a dilute Ba(OH)2 solution if (a) 50.00 mL yielded 0.1791 g of BaSO4. (b) titration of 0.4512 g of primary standard potassium hydrogen phthalate (KHP) required 26.46 mL of the base. (c) addition of 50.00 mL of the base to 0.3912 g of benzoic acid required a 4.67-mL back-titration with 0.05317 M HCl.arrow_forward(a) If the molar solubility of Mg3(PO4)2 at 25 oC is 6.26e-06 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 0.00336 g of Ag2C2O4 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Ag2C2O4.Ksp = (c) The Ksp of Sc(OH)3 at 25 oC is 2.22e-31. What is the molar solubility of Sc(OH)3?solubility = mol/Larrow_forwardAluminum hydroxide reacts with an excess of hydroxide ions to form the complex ionAl(OH)4-.(a) Write an equation for this reaction.(b) Calculate K.(c) Determine the solubility of Al(OH)3(in mol/L) at pH 12.0.arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY