General Chemistry Questions on Acids/Bases/Salts – Calculations (includes Balancing Redox

**1.**How many grams of Ca(OH)_{2}are contained in 1500 mL of 0.0250 M Ca(OH)_{2}solution?- (a) 3.17 g
- (b) 2.78 g
- (c) 1.85 g
- (d) 2.34 g
- (e) 4.25 g
**2.**What volume of 12.6 M HCl must be added to enough water to prepare 5.00 liters of 3.00 M HCl?- (a) 1.19 L
- (b) 21.0 L
- (c) 0.840 L
- (d) 7.56 L
- (e) 2.14 L
**3.**What is the molarity of the salt produced in the reaction of 200 mL of 0.100 M HCl with 100 mL of 0.500 M KOH?- (a) 0.0325 M
- (b) 0.0472 M
- (c) 0.0667 M
- (d) 0.0864 M
- (e) 0.0935 M
**4.**What volume of 0.50 M KOH would be required to neutralize completely 500 mL of 0.25 M H_{3}PO_{4}solution?- (a) 2.5 x 10
^{2}mL - (b) 1.4 x 10
^{3}mL - (c) 83 mL
- (d) 7.5 x 10
^{2}mL - (e) 5.2 x 10
^{2}mL **5.**A 0.6745 gram sample of KHP reacts with 41.75 mL of KOH solution for complete neutralization. What is the molarity of the KOH solution? (Molecular weight of KHP = 204 g/mol. KHP has one acidic hydrogen.)- (a) 0.158 M
- (b) 0.099 M
- (c) 0.139 M
- (d) 0.079 M
- (e) 0.061 M
**6.**How many equivalents of phosphoric acid are contained in 300 mL of 4.00 M phosphoric acid? (Assume the acid is to be completely neutralized by a base.)- (a) 0.600 eq
- (b) 1.20 eq
- (c) 2.40 eq
- (d) 3.60 eq
- (e) 4.80 eq
**7.**Calculate the normality of a solution that contains 4.5 g of (COOH)_{2}in 3000 mL of solution? (Assume the (COOH)_{2}is to be completely neutralized in an acid-base reaction.)- (a) 0.033 N
- (b) 0.045 N
- (c) 0.066 N
- (d) 0.090 N
- (e) 0.12 N
**8.**What volume of 0.100 N HNO_{3}is required to neutralize 50.0 mL of a 0.150 N solution of Ba(OH)_{2}?- (a) 50.0 mL
- (b) 75.0 mL
- (c) 100. mL
- (d) 125 mL
- (e) 150. mL
**9.**How many grams of NaOH would be required to neutralize all the acid in 75.0 mL of 0.0900 N H_{2}SO_{4}?- (a) 0.540 g
- (b) 0.270 g
- (c) 1.32 g
- (d) 0.660 g
- (e) 0.859 g
**10.**What is the oxidation number for carbon in CaC_{2}O_{4}?- (a) 0
- (b) +2
- (c) +3
- (d) +4
- (e) +6
**11.**Balance the molecular equation for the following redox reaction. What is the sum of the coefficients? Don’t forget coefficients of one. Use the smallest whole number coefficients possible.H _{2}SO_{4}(aq) + HI(aq) I_{2}(s) + SO_{2}(g)- (a) 7
- (b) 9
- (c) 11
- (d) 13
- (e) 5
**12.**For the reaction between permanganate ion and sufite ion in basic solution, the unbalanced equation is:MnO _{4}^{–}+ SO_{3}^{2-}MnO_{2}+ SO_{4}^{2-}

When this equation is balanced using the smallest whole number coefficients possible, the number of OH^{–}ions is- (a) two on the right.
- (b) two on the left.
- (c) three on the right.
- (d) four on the right.
- (e) four on the left.
**13.**Balance the following redox equation in acidic solution with the smallest whole number coefficients possible. What is the sum of all the coefficients? (Do not forget coefficients of one.)Cu + SO _{4}^{2-}Cu^{2+}+ SO_{2}(in acidic solution)- (a) 9
- (b) 10
- (c) 11
- (d) 12
- (e) 13
**14.**When the following equation is balanced with the smallest possible set of integers, what is the sum of all the coefficients? (Do not forget coefficients of one.)Cr _{2}O_{7}^{2-}+ H_{2}S Cr^{3+}+ S (in acidic solution)- (a) 13
- (b) 24
- (c) 19
- (d) 7
- (e) 29
**15.**When the following equation is balanced with the smallest possible set of integers, what is the sum of all the coefficients? (Do not forget coefficients of one.)MnO _{4}^{–}+ Se^{2-}MnO_{2}+ Se (in basic solution)- (a) 20
- (b) 22
- (c) 24
- (d) 26
- (e) 28
**16.**Consider the following**unbalanced**equation in acidic solution:NaClO A 25.0 mL sample of 0.0833 M NaClO_{3}+ H_{2}O + I_{2}HIO_{3}+ NaCl_{3}reacted with 30.0 mL of an aqueous solution of I_{2}. How many grams of I_{2}were contained in the I_{2}solution?- (a) 0.264 g
- (b) 0.397 g
- (c) 0.236 g
- (d) 0.159 g
- (e) 0.317 g
**17.**Consider the following unbalanced net ionic equation:NO What is the molarity of a sodium nitrite, NaNO_{2}^{–}+ MnO_{4}^{–}NO_{3}^{–}+ Mn^{2+}(in acidic solution)_{2}, solution if 30.0 mL of it just reacts with 0.238 grams of KMnO_{4}?- (a) 0.410 M
- (b) 0.126 M
- (c) 0.0502 M
- (d) 0.251 M
- (e) 0.0316 M
**18.**What is the equivalent weight (in grams) of copper(II) nitrate for use in a reaction involving the conversion of copper(II) to copper metal?- (a) 46.9 g/eq
- (b) 93.8 g/eq
- (c) 187.6 g/eq
- (d) 375.2 g/eq
- (e) 562.8 g/eq
**19.**What is the normality of a K_{2}Cr_{2}O_{7}solution prepared by dissolving 5.00 g of K_{2}Cr_{2}O_{7}in 200 mL of solution, which will be used in the following**unbalanced**reaction?Cr _{2}O_{7}^{2–}+ SO_{3}^{2–}Cr^{3+}+ SO_{4}^{2–}(in acidic solution)- (a) 0.733 N
- (b) 0.226 N
- (c) 0.510 N
- (d) 0.441 N
- (e) 0.810 N
**20.**What mass of KMnO_{4}must be dissolved to prepare 1.25 L of 0.110 N KMnO_{4}solution? It is used in the reaction in which MnO_{4}^{–}ions oxidize Fe^{2+}into Fe^{3+}ions and are reduced to Mn^{2+}ions under acidic conditions?- (a) 4.34 g
- (b) 23.8 g
- (c) 115 g
- (d) 19.1 g
- (e) 70.6 g
**21.**A 0.250 M solution of Na_{2}C_{2}O_{4}is to be used in a reaction in which the C_{2}O_{4}^{2–}will be oxidized to CO_{2}. What is the normality of this Na_{2}C_{2}O_{4}solution?- (a) 0.250 N
- (b) 1.00 N
- (c) 0.125 N
- (d) 0.0625 N
- (e) 0.500 N
**22.**What volume of a 0.150 N KI solution is required to react in basic solution with 34.1 mL of a 0.216 N solution of KMnO_{4}? The products in the reaction include MnO_{2}and IO_{3}^{–}.- (a) 25.4 mL
- (b) 37.9 mL
- (c) 12.6 mL
- (d) 98.2 mL
- (e) 49.1 mL
**23.**Calculate the normality of a NaClO solution if 35.00 mL of the solution is required to react with 0.615 g of Zn according to the following unbalanced equation:Zn + ClO ^{–}Zn(OH)_{2}+ Cl^{–}(in basic solution)- (a) 0.537 N
- (b) 0.275 N
- (c) 0.108 N
- (d) 0.366 N
- (e) 0.791 N
**24.**A solution of nitrous acid was standardized in a reaction where HNO_{2}NO_{3}^{–}and its concentration was determined to be 0.100 N nitrous acid. What volume of this 0.100 N nitrous acid solution would be required to oxidation of 0.200 g of CoCl_{2}to CoCl_{3}according to the following net ionic equation?Co ^{2+}+ HNO_{2}Co^{3+}+ NO (in acidic solution)- (a) 33.9 mL
- (b) 15.4 mL
- (c) 7.70 mL
- (d) 67.8 mL
- (e) 30.8 mL
**25.**What is the sum of all coefficients when the following net ionic equation is balanced using the smallest whole number coefficients possible? Do not forget coefficients of one.MnO _{4}^{–}+ Mn^{2+}MnO_{2}(in basic solution)- (a) 19
- (b) 16
- (c) 13
- (d) 11
- (e) 7

**Answers:**

**1.** (b)** 2.** (a) **3.** (c) **4.** (d)** 5.** (d) **6.** (d) **7.** (a)** 8.** (b)** 9.** (b) **10.** (c) **11.** (a) **12.** (a) **13.** (b) **14.** (b) **15.** (b) **16.** (e) **17.** (b)** 18.** (b)** 19.** (c) **20.** (a) **21.** (e) **22.** (e) **23.** (a) **24.** (e) **25.** (b)