University:
Arizona State University
Course:
CHM 101 | Introductory Chemistry
Academic year:

2020
Views:

274

Pages:

3
Author:

Carissa Thomas

Acids & Bases Review 1. Name the following compounds as acids and circle which are weak acids: a) HNO3 nitric acid b) H2SO4 sulfuric acid c) HF hydrofluoric acid d) H2CO3 carbonic acid 2. Write the formulas for the following bases: a) calcium hydroxide b) aluminum hydroxide Ca(OH)2 Al(OH)3 e) HC2H3O2 acetic acid f) H3PO4 phosphoric acid c) ammonium hydroxide d) lithium hydroxide NH4OH LiOH 3. Complete the following table: Acids A substance that increases the concentration of H+ (or H3O+) when added to water. Definition Bases A substance that increases the concentration of OH— when added to water. or A substance that acts as a proton (H+) donor. Electrolyte in aqueous solution? or A substance that acts as a proton (H+) acceptor. H+ pH less than 7 Taste Litmus turns Which reacts with metals to form H2 gas? OH— greater than 7 sour bitter blue turns red red turns blue yes no Conjugate acid-base pairs: 4. Identify the acid, the base, the conjugate acid and the conjugate base in the reactions: NH3 (g) + H2O (l) NH4+(aq) + OH-(aq) base acid conj. acid conj. base CO32~ (aq) + H3O+ (aq) HCO3~ (aq) + H2O (l) acid base conj. base conj. acid 5. An acid will form the conjugate _base_and a base will form the conjugate _acid__. Neutralization: 6. Classify the following acids as monoprotic, diprotic or triprotic: a) H2SO4 diprotic b) H3PO4 c) HCl triprotic monoprotic d) HC2H3O2 or CH3COOH (same thing) monoprotic 7. What is the concentration of an unknown NaOH solution if it took an average of 15.4 mL of 0.100 M HCl solution to neutralize 10.0 mL of the NaOH solution? balanced chemical reaction: HCl + NaOH à NaCl + H2O 7&8 =1.54×10;< &moles moles&of&HCl&used=c×V=0.100&M&×&15.4&mL× 7999&:8 7&:@A&BCDE =1.54×10;< &moles moles&of&NaOH= moles&of&HCl× 7&:@A&EFA :@AHI&BCDE conc. of&NaOH= J&BCDE&KIHL= 7.MN×79OP 9.97999&8 =0.154&M pH/pOH calculations: 8. A solution has a [H3O+] of 1×10;Q M, what is its pH?____Is this an acid, base or neutral? pH= −logH< OU = −log1×10;Q =7 9. What is the pH of a solution if the [H+] = 7.2×10;X M?_____ Is this an acid or base? pH= −logH< OU = −log7.2×10;X =8.1 10. If the pH of a solution is 0.8, what is its hydronium ion concentration? ___________ H< OU = 10;ZE = 10;9.[ =0.2&M 11. What is the pH of a 1.0 M HCl solution? ______ Would this turn litmus paper red or blue? HCl à H+ + Cl— (strong acids fully ionize in water) pH= −logH< OU = −log1.0 =0 12. What is the pH of a solution if the [OH —] = 2.0×10;M M? __________ pH= −logOH ; = −log2.0×10;M =4.7 pH+ pOH= 14 pOH= 14− pH= 14−4.7 = 9.3 13. If the [H+] of a solution is 2.5×10;N M, what is the concentration of the hydroxide ion?_____ Is this solution an acid or a base? K ` = [H U ][OH; ] =1.0×10;7N [OH ; ] = 7.9×79 Ocd e.M×79 Od =4.0×10;77 Ionization of acids and bases: 14. Write the expression for the acid dissociation constant of the strong acid HBr HBr à H+ + Br— KC = Ef [ghO ] [Egh] 15. A 0.10 M solution of formic acid, HCOOH, has an equilibrium [H+] = 4.2×10;< M. What is the Ka of formic acid? The equilibrium is shown below: H+ (aq) HCOOH (aq) + HCOO-(aq) initial 0.10 M 0 0 change −x +x +x 0.10−x equilibrium =0.10−4.2×10;< =0.096 M KC = 0+x 0+x =4.2×10;< M =4.2×10;< M H U HCOO; HCOOH 4.2×10;< e 6 =1.8×10; note: can use [HCOOH]≈0.10 M at equilibrium