Chemistry Acid/Base worksheet

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I need the answers to this acid and base worksheet to study. It is intro chemistry and you do not need to do question 14. If you could show work when needed! thanks!

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Acid/Base Chemistry: Extra Credit Assignment (due by Thursday, 5/10) H2CO3 (aq) + H2O (l) → HCO3- (aq) + H3O+ (aq) 1) a) What role is H2O playing in this reaction? acid base b) What role is H2CO3 playing in this reaction? acid base c) Which reactant is acting as a proton donor? _______________________________ d) Which reactant is acting as a proton acceptor? _______________________________ e) What are the two conjugate acid/base pairs in the reaction? ________________ /________________ and _____________ / _______________ CN- (aq) + H2O (l) → HCN (aq) + OH- (aq) 2) a) What role is H2O playing in this reaction? acid base b) What role is CN- playing in this reaction? acid base c) Which reactant is acting as a proton donor? _______________________________ d) Which reactant is acting as a proton acceptor? _______________________________ e) Complete the following statements: • • • • CN- is the conjugate _______________ of HCN HCN is the conjugate ______________ of CNH2O is the conjugate ______________ of OHOH- is the conjugate ______________ of H2O H2PO4- (aq) + H2O (l) → HPO42- (aq) + H3O+ (aq) 3) a) What role is H2O playing in this reaction? acid base b) What role is H2PO4- playing in this reaction? acid base c) Complete the following statements: • • • • H3O+ is the conjugate ______________ of H2O H2O is the conjugate ______________ of H3O+ HPO42- is the conjugate ________________ of H2PO4H2PO4- is the conjugate ________________ of HPO42- 4) For each of the following substances, write a balanced chemical equation showing it acting as a Bronsted-Lowry acid or base in aqueous solution. Show all phases! (Remember that for weak acids and bases, equilibrium arrows (→) are used to indicate that the reaction isn’t going to completion.) a) HBr (acting as strong acid) b) OCl- (acting as a weak base) c) H2SO3 (acting as a weak acid) d) CH3NH2 (acting as a weak base) 5) What is the conjugate base of each of the following substances? Pay close attention to the charge! HCl ___________________ HBr ___________________ HF _______________ HNO3 ___________________ H2SO4 ___________________ H3PO4 ______________ HCO3- ___________________ HPO42- ___________________ H3O+ _____________ 6) What is the conjugate acid of each of the following substances? Again, pay close attention to getting the correct charge in your answer. OH- ________________ NH3 __________________ H2O __________________ I- ________________ HSO4- __________________ IO3- ___________________ H2PO4- ________________ CO32- __________________ PO43- ___________________ 7) Classify each of the acids below as strong (ionizing completely) or weak (ionizing partially). HCl ________________ HBr _________________ HF __________________ HNO3 ________________ HNO2 _________________ HCN __________________ H2SO3 ________________ H2SO4 _________________ H2CO3 __________________ H3PO4 ________________ HClO4 _________________ HIO3 8) __________________ Classify each of the bases below as strong (ionizing completely) or weak (ionizing partially). NaOH ________________ NH3 _________________ KOH __________________ CH3NH2 ________________ Ca(OH)2 _________________ CN- __________________ LiOH ________________ CH3CH2NH2 ______________ F- __________________ 9) For the following solutions, you are given the molarity of the hydronium ion, [H3O+]. Calculate the molarity of the hydroxide ion, [OH-], to 2 sig figs and then classify the solution as either acidic or basic. Remember, [H3O+] [OH-] = 1.0 x 10-14 a) [H3O+] = 1.2 x 10-4 M [OH-] = ________________________ M acidic basic b) [H3O+] = 5.8 x 10-11 M [OH-] = ________________________ M acidic basic c) [H3O+] = 7.5 x 10-3 M [OH-] = ________________________ M acidic basic d) [H3O+] = 8.2 x 10-6 M [OH-] = ________________________ M acidic basic e) [H3O+] = 3.7 x 10-9 M [OH-] = ________________________ M acidic basic f) [H3O+] = 6.2 x 10-13 M [OH-] = ________________________ M acidic basic 10) 11) 12. What is the pH of each of the solutions in Problem #9? (Report each pH value to the 2 nd decimal place.) Remember, pH = - log [ H3O+] a) pH = _______________________ d) pH = ______________________ b) pH = _______________________ e) pH = ______________________ c) pH = _______________________ f) pH = ______________________ For each of the pH values given below, first classify the solution as acidic or basic. Then calculate the value of [H3O+] for each of the solutions to two sig figs. Remember, [H3O+] = 10-pH a) pH = 12.69 acidic basic [H3O+] = _______________________ M b) pH = 6.42 acidic basic [H3O+] = _______________________ M c) pH = 2.35 acidic basic [H3O+] = _______________________ M d) pH = 8.84 acidic basic [H3O+] = _______________________ M e) pH = 4.56 acidic basic [H3O+] = _______________________ M A solution has a hydroxide ion concentration, [OH-], of 0.075 M. a) Showing your work, calculate [H3O+] for the solution. b) Showing your work, calculate the pH of the solution. c) Is this solution acidic or basic? ___________________________ 13) Consider a 0.50 M solution of HCl, a strong acid. a) What is the value of [H3O+] for the solution? b) What is the value of [OH-] for the solution? (Show your calculation below.) c) What is the pH of the solution? 14) Now, consider a 0.50 M solution of HF, a weak acid. In this course, we don’t know how to calculate pH for a weak acid (or weak base), but we should be able to compare this this solution to a strong acid, such as 0.50 M HCl. a) Is 0.50 M HF more acidic or less acidic than 0.50 M HCl? more acidic less acidic b) Which solution has a higher pH value? 0.50 M HF 0.50 M HCl c) Which solution has a higher concentration of [H3O+]? 0.50 M HF 0.50 M HCl d) Which solution has a higher concentration of [OH-]? 0.50 M HF 0.50 M HCl 15) A solution has a pH of 9.44. Showing your work, calculate the values of [H3O+] and [OH-] for the solution. [H3O+] = _______________________ M __________________ ____________________ [OH-] = _________________________ M
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