South Carolina State University

Department of Physical Sciences, SGCH11, NH, Name

VERSION 1

1. A 0.742-gram sample of KHP, KC•H4(COO)(COOH), reacts with 35.0 mL of Ba(OH)2 solution. What is the

molarity of the Ba(OH)2 solution?

a) 0.127 M b) 0.0636 M c) 0.0520 M d) 0.208 M e) 0.104 M

2. If 400. mL of 0.20 M HCl solution is added to 800. mL of 0.050 M Ba(OH2 solution, the resulting solution will be

__________ in BaCl2.

a) 0.067 M b) 0.26 M c) 0.033 M d) 0.47 M e) 0.67 M

3. What mass of BaSO4 will be produced by the reaction of excess BaCl2 with 50.0 mL of 0.400 N H2SO4 solution?

H2SO4 + BaCl2 → BaSO4(s) + 2HCl

a) 9.32 g b) 10.4 g c) 4.66 g d) 6.72 g e) 2.33 g

4. What is the molarity of the NaBr produced when 50.0 mL of 4.80 M NaOH is mixed with 150.0 mL of 1.60 M HBr?

a) 2.40 M b) 3.20 M c) 1.20 M d) 1.33 M e) 480 M

5. What is the molarity of 600. mL of solution containing 6.72 grams of sulfuric acid?

a) 0.114 M b) 0.288 M c) 0.342 M d) 0.180 M e) 0.360 M

6. In acidic solution MnO4

- oxidizes H3AsO3, a weak acid, to H3AsO4, a weak acid, and is reduced to Mn2+. Write the

balanced net ionic equation for this reaction. How many H+ are there in the balanced equation?

a) 1 b) 6 c) 4 d) 3 e) 2

7. During a titration the point at which stoichiometrically equivalent amounts of acid and base have reacted is called the

___________ point.

a) indicator b) primary standard c) standardization d) end e) equivalence

8. What is the molarity of a barium hydroxide solution if 18.62 mL of this Ba(OH)2 solution requires 35.84 mL of

0.2419 M HCl for titration to the equivalence point?

a) 0.4656 M b) 0.2328 M c) 0.1164 M d) 0.3492 M e) 0.6984 M

9. Balance the following equation. How many HCl are there on the left side of the balanced equation?

K2Cr2O– + Na2SO3 + HCl → KCl + Na2SO4 + CrCl3 + H2O

a) 1 b) 8 c) 4 d) 3 e) 2

10. How many grams of AgNO3 are needed to make 500. mL of 0.200 M solution?

a) 170. g b) 85000 g c) 34.0 g d) 85.0 g e) 17.0 g

11. Balance the following net ionic equation. Use H+ rather than H3O+. What is the sum of the coefficients?

I- + NO2

- → NO + I2 (acidic solution)

a) 11 b) 19 c) 17 d) 15 e) 13

12. Chlorous acid, HClO2, oxidizes sulfur dioxide, SO2, to sulfate ions, SO4

2- and is reduced to chloride ions, Cl-, in

acidic solution. Use H+ rather than H3O+. Write the balanced net ionic equation for the reaction. What is the sum

of the coefficients?

a) 11 b) 19 c) 17 d) 15 e) 13

13. Balance the following net ionic equation. What is the coefficient of OH-?

MnO4

- + NH3 Ä¢ NO3

- + MnO2 (basic solution)

a) 2 b) 9 c) 7 d) 5 e) 3

Partial preview of the text

Download Test 7 with Answer Key - General Chemistry II | C 152 and more Exams Chemistry in PDF only on Docsity!

South Carolina State University Department of Physical Sciences, SGCH11, NH, Name VERSION 1

A 0.742-gram sample of KHP, KC•H 4 (COO)(COOH), reacts with 35.0 mL of Ba(OH) 2 solution. What is the molarity of the Ba(OH) 2 solution? a) 0.127 M b) 0.0636 M c) 0.0520 M d) 0.208 M e) 0.104 M
If 400. mL of 0.20 M HCl solution is added to 800. mL of 0.050 M Ba(OH 2 solution, the resulting solution will be __________ in BaCl 2. a) 0.067 M b) 0.26 M c) 0.033 M d) 0.47 M e) 0.67 M
What mass of BaSO 4 will be produced by the reaction of excess BaCl 2 with 50.0 mL of 0.400 N H 2 SO 4 solution? H 2 SO 4 + BaCl 2 → BaSO 4 (s) + 2HCl a) 9.32 g b) 10.4 g c) 4.66 g d) 6.72 g e) 2.33 g
What is the molarity of the NaBr produced when 50.0 mL of 4.80 M NaOH is mixed with 150.0 mL of 1.60 M HBr? a) 2.40 M b) 3.20 M c) 1.20 M d) 1.33 M e) 480 M
What is the molarity of 600. mL of solution containing 6.72 grams of sulfuric acid? a) 0.114 M b) 0.288 M c) 0.342 M d) 0.180 M e) 0.360 M
In acidic solution MnO 4 -^ oxidizes H 3 AsO 3 , a weak acid, to H 3 AsO 4 , a weak acid, and is reduced to Mn2+. Write the balanced net ionic equation for this reaction. How many H+^ are there in the balanced equation? a) 1 b) 6 c) 4 d) 3 e) 2
During a titration the point at which stoichiometrically equivalent amounts of acid and base have reacted is called the ___________ point. a) indicator b) primary standard c) standardization d) end e) equivalence
What is the molarity of a barium hydroxide solution if 18.62 mL of this Ba(OH) 2 solution requires 35.84 mL of 0.2419 M HCl for titration to the equivalence point? a) 0.4656 M b) 0.2328 M c) 0.1164 M d) 0.3492 M e) 0.6984 M
Balance the following equation. How many HCl are there on the left side of the balanced equation? K 2 Cr 2 O– + Na 2 SO 3 + HCl → KCl + Na 2 SO 4 + CrCl 3 + H 2 O a) 1 b) 8 c) 4 d) 3 e) 2
How many grams of AgNO 3 are needed to make 500. mL of 0.200 M solution? a) 170. g b) 85000 g c) 34.0 g d) 85.0 g e) 17.0 g
Balance the following net ionic equation. Use H+^ rather than H 3 O+. What is the sum of the coefficients? I-^ + NO 2 -^ → NO + I 2 (acidic solution) a) 11 b) 19 c) 17 d) 15 e) 13
Chlorous acid, HClO 2 , oxidizes sulfur dioxide, SO 2 , to sulfate ions, SO 4 2-^ and is reduced to chloride ions, Cl-, in acidic solution. Use H+^ rather than H 3 O+. Write the balanced net ionic equation for the reaction. What is the sum of the coefficients? a) 11 b) 19 c) 17 d) 15 e) 13
Balance the following net ionic equation. What is the coefficient of OH-? MnO 4 -^ + NH 3 Ä¢ NO 3 -^ + MnO 2 (basic solution) a) 2 b) 9 c) 7 d) 5 e) 3

A 25.0-mL sample of 0.0833 M NaClO 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? NaClO 3 + H 2 O + I 2 → HIO 3 + NaCl (unbalanced) a) 0.264 g b) 0.317 g c) 0.159 g d) 0.236 g e) 0.397 g
What is the oxidation number of S in Na 2 SO 3 .12H 2 O? a) +6 b) +5 c) +4 d) +3 e) +
Balance the following net ionic equation. What is the sum of the coefficients? MnO 4 -^ + I-^ + H 2 O Æ I 2 + MnO 2 + OH- a) 21 b) 29 c) 27 d) 25 e) 23
In which of the following is the oxidation number of the underlined element given incorrectly? oxidation number oxidation number oxidation number a) K 2 Cr 2 O– +6 c) HIO 4 +5 d) (NH 4 ) 2 SO 4 + b) NaAl(OH) 4 +3 e) NaHSO 3 +
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) 2.14 L c) 7.56 L d) 0.840 L e) 21.0 L
What volume of 0.100 M (COOH) 2 solution would be required to react with 0.164 grams of KMnO 4? 5(COOH) 2 + 2MnO 4 -^ + 6H+^ → 10CO 2 + 2Mn2+^ + 8H 2 O a) 25.9 mL b) 90.8 mL c) 104 mL d) 77.8 mL e) 51.8 mL
Balance the following formula unit equation. What is the sum of all of the coefficients? KMnO 4 + H 2 O 2 + H 2 SO 4 → O 2 + MnSO 4 + K 2 SO 4 + H 2 O a) 22 b) 30 c) 28 d) 26 e) 24
How many H 2 O are there in the balanced equation? CuS + NO 3 -^ + H+^ → Cu‚+^ + S + NO + H 2 O a) one b) five c) four d) three e) two
An impure 0.500 7 gram sample of FeSO 4 reacts with 20.0 mL of 0.0200 M KMnO 4. Assuming that the impurities do not react with KMnO 4 , what is the percentage of FeSO 4 in the sample? MnO 4 -^ + 8H+^ + 5Fe‚+^ Æ Mn2+^ + 5Fe3+^ + 4H 2 O a) 52.3% b) 69.2% c) 64.5% d) 60.8% e) 56.6%
What is the molarity of a Na 2 Cr 2 O– solution if 22.5 mL of it is required to oxidize 33.0 mL of 0.150 M Fe(NH 4 ) 2 (SO 4 ) 2? The reaction products include Cr„+^ and Fe„+. a) 0.184 M b) 0.220 M c) 0.0367 M d) 0.0440 M e) 0.0660 M
If 38.46 mL of KOH solution is required to titrate 22.68 mL of 0.1088 N H 3 PO 4 solution, what is the normality of the KOH solution? (Assume the acid is completely neutralized by the base.) a) 0.1925 N b) 0.1604 N c) 0.1283 N d) 0.09624 N e) 0.06416 N
What is the normality of 150. mL of a solution that contains 5.00 grams of H 3 PO 4? (Assume the acid is to be completely neutralized.) a) 1.02 N b) 0.870 N c) 0.340 N d) 0.113 N e) 0.667 N

Test 7 with Answer Key - General Chemistry II | C 152, Exams of Chemistry

Related documents

Partial preview of the text

Download Test 7 with Answer Key - General Chemistry II | C 152 and more Exams Chemistry in PDF only on Docsity!