15. The mixing of which pair of reactants will result in a precipitation reaction?
CsI(aq) + NaOH(aq)
HCl(aq) + Ca(OH)2(aq)
K2SO4(aq) + Hg2(NO3)2(aq)
NaNO3(aq) + NH4Cl(aq)
16. Which of the following is a precipitation reaction?
Zn(s) + 2 AgNO3(aq) 2 Ag(s) + Zn(NO3)2(aq)
NaCl(aq) + LiI(aq) NaI(aq) + LiCl(aq)
2 KI(aq) + Hg2(NO3)2(aq) Hg2I2(s) + 2 KNO3(aq)
HI(aq) + NaOH(aq) NaI(aq) + H2O(l)
None of these are precipitation reactions.
17. Which of the following pairs of aqueous solutions will form a precipitate when mixed?
K2CO3 + NaBr
Na2 SO4 + KOH
CaS + Na2SO4
None of these solution pairs will produce a precipitate.
All of these solution pairs will produce a precipitate.
18. Which of the following pairs of aqueous solutions will form a precipitate when mixed?
NH4NO3 + Li2CO3
Hg2(NO3)2 + LiCl
NaCl + Li3PO4
AgC2H3O2 + Cu(NO3)2
None of these solution pairs will produce a precipitate.
19. Silver ions can be precipitated from aqueous solutions by the addition of aqueous chloride:
Silver chloride is virtually insoluble in water so that the reaction appears to go to completion. How many grams of solid NaCl must be added to 25.0 mL of 0.366 M AgNO3 solution to completely precipitate the silver?
9.15 × 10-3 g
1.57 × 10-4 g
0.535 g
0.157 g
6.39 × 103 g
20.Identify the polyprotic acid.
H2SO4
HCl
LiCl
LiOH
Ca(OH)2
21.In an acid-base neutralization reaction 38.74 mL of 0.500 M potassium hydroxide reacts with 50.00 mL of sulfuric acid solution. What is the concentration of the H2SO4 solution?
0.194 M
0.387 M
0.775 M
1.29 M
22. A solution is prepared by mixing 50.0 mL of 0.100 M HCl and 10.0 mL of 0.200 M NaCl. What is the molarity of chloride ion in this solution?
0.183
8.57
3.50
0.0500
0.117
23. A solution is prepared by adding 1.60 g of solid NaCl to 50.0 mL of 0.100 M CaCl2. What is the molarity of chloride ion in the final solution? Assume that the volume of the final solution is 50.0 mL.
0.747
0.647
0.132
0.232
0.547
24. What is the molarity of a NaOH solution if 28.2 mL of a 0.355 M H2SO4 solution is required to neutralize a 25.0-mL sample of the NaOH solution?
0.801
0.315
0.629
125
0.400
25. What is the oxidation number of the sulfur atom in K2SO4 ?
-2
+2
+4
+6
26.Determine the oxidation state of S in Na2SO4.
-4
+2
+4
+6
-2
27. Identify the oxidation state of Ba in Ba(s).
+1
+2
0
-1
-2
28. Balance the chemical equation given below, and determine the number of grams of MgO are needed to produce 10.0 g of Fe2O3.
0.312 g
0.841 g
2.52 g
7.57 g
29. If the density of ethanol, C2H5OH, is 0.789 g/mL. How many milliliters of ethanol are needed to produce 15.0 g of CO2 according to the following chemical equation?
6.19 mL
9.95 mL
19.9 mL
39.8 mL
30. If the percent yield for the following reaction is 75.0%, and 45.0 g of NO2 are consumed in the reaction, how many grams of nitric acid, HNO3(aq) are produced?
30.8 g
41.1 g
54.8 g
69.3 g
31. Determine the theoretical yield of H2S (in moles) if 64 mol Al2S3 and 64 mol H2O are reacted according to the following balanced reaction. A possibly useful molar mass is Al2S3 = 150.17 g/mol.
192 mol H2S
64 mol H2S
128 mol H2S
96 mol H2S
32 mol H2S
32. Which substance is the limiting reactant when 2.0 g of sulfur reacts with 3.0 g of oxygen and 4.0 g of sodium hydroxide according to the following chemical equation
S(s)
O2(g)
NaOH(aq)
None of these substances is the limiting reactant.
15. The mixing of which pair of reactants will result in a precipitation reaction? CsI(aq)...
(7. Consider the reaction as follows: Na2SO4(aq) + BaCl2(aq) → BaSO4(s) + 2 NaCl(aq) A 1.00-mol sample of sodium sulfate was placed into the barium chloride aqueous solution to make solid barium sulfate. (a) How many gram of sodium sulfate was placed into the reaction solution? (b) What is the maximum mass of NaCl formed? (c) If 78.9 g of NaCl was obtained, what was the percent yield of NaCl? 3. How many liters of 0.186 M of NaOH (aq)...
The mixing of which pair of reactants will result in a precipitation reaction? K2SO4(aq) + Sr(NO3)2(aq) HCl(aq) + Ca(OH)2(aq) NaNO3(aq) + NH4Cl(aq) CsI(aq) + NaOH(aq) Submit Request Answer
A solution of NaCl(aq) is added slowly to a solution of lead nitrate, Pb(NO3)2(aq), until no further precipitation occurs. The precipitate is collected by filtration, dried, and weighed. A total of 15.59 g PbCl2(s) is obtained from 200.0 mL of the original solution. Calculate the molarity of the Pb(NO3)2(aq) solution. concentration: M
Question 1 According to the following reaction, what mass of silver nitrate would be required to react with 0.500 grams of potassium chloride? AgNO3 (aq) + KCl (aq) --> AgCl (s) + KNO3 (aq) options 2.68 g 0.500 g 85.0 g 170 g 1.14 g Question 2 Consider the reaction: Na2CO3 (aq)+ 2 HCl (aq) --> 2 NaCl (aq) + CO2 (g) + H2O (l) If 43.41 g of sodium carbonate react completely, how many grams of HCl will be...
In a precipitation reaction between Al(NO3)3(aq) and Na2S(aq), 12.7 mL of 0.150 M Al(NO3)3(aq) completly reacted with 10.5 mL of Na2S(aq). What was the molarity of Na2S(aq)? 2 Al(NO3)3(aq) + 3 Na2S(aq) → Al2S3(s) + 6 NaNO3(aq) Note: Insert only the numerical value of your answer with three decimal places (do not include the units or chemical in your answer).
By titration, it is found that 91.9 mL of 0.150 M NaOH(aq) is needed to neutralize 25,0 mL of HCl(aq). Calculate the concentration of the HCl solution. HCl concentration: A solution of NaCl(aq) is added slowly to a solution of lead nitrate, Pb(NO3)2(aq), until no further precipitation occurs. The precipitate is collected by filtration, dried, and weighed. A total of 19.42 g PbCl(s) is obtained from 200.0 mL of the original solution. Calculate the molarity of the Pb(NOx),(aq) solution. concentration:
A solution of NaCl(aq) is added slowly to a solution of lead nitrate, Pb(NO3)2(aq) Pb ( NO 3 ) 2 ( aq ) , until no further precipitation occurs. The precipitate is collected by filtration, dried, and weighed. A total of 10.47 g PbCl2(s) 10.47 g PbCl 2 ( s ) is obtained from 200.0 mL 200.0 mL of the original solution. Calculate the molarity of the Pb(NO3)2(aq) Pb ( NO 3 ) 2 ( aq ) solution. concentration: M
8. A solution of NaCl(aq) is added slowly to a solution of lead nitrate, Pb(NO3)2(aq), until no further precipitation occurs. The precipitate is collected by filtration, dried, and weighed. A total of 12.12 g PbCl2(s) is obtained from 200.0 mL of the original solution. Calculate the molarity of the Pb(NO3)2(aq) solution. concentration: M
Silver ions can be precipitated from aqueous solutions by the addition of aqueous chloride: Ag+(aq)+Cl−(aq)→AgCl(s) Silver chloride is virtually insoluble in water so that the reaction appears to go to completion. How many grams of solid NaCl must be added to 25.0 mL of 0.149 M AgNO3 solution to completely precipitate the silver?
Which of the following reactions could be considered a "precipitation" reaction? NaOH(aq) + HCl(aq) + NaCl(aq) + H2O(1) 2H2O(1) + 2H2(g) + O2(g) + 2Nal(aq) + Pb(NO3)2(aq) + 2NaNO3(aq) + Pbl2(s) 2C2H6(g) + 702(g) + 4CO2(g) + 6H2O(1) None of these