Chem 103 Final Exam | Verified Exam Questions and Answers | Latest
Updated Study Material 2026
Question:
Which of the following are weak electrolytes? HCl HC2H3O2 NH3 KCl CH3OH
Answer:
Answers: HC2H3O2 & NH3
Question:
Explanation
Answer:
Weak acids and bases
Question:
A solution has a pH of 4.0. If a second solution has a pH of 8.0, what is the ratio of hydrogen ion ion
concentration in solution 1 compared to solution 2?
Answer:
Answer: 10,000
Question:
What is the hydroxide ion concentration in a solution with a pH of 6.0?
Answer:
Answer: 1.0 x 10^-8 M
Question:
Explanation
Answer:
We know the pH of the solution is 6.0 We can find OH from this formula: OH- = 14- pH Plug in pH to
find hydroxide ion concentration: OH- = 14-6 = 8 So, 1.0 x 10^-8 M
Question:
Which of the following weak acid dissociation constants would result in the least ionization?
Answer:
Answer: Ka = 1.0 x 10^-5
, Question:
If 10.0 mL of an HBr solution with a pH of 4 is diluted to a total volume of 1.0 L what is the pH of the 1
L solution?
Answer:
Answer: 6.0
Question:
Explanation
Answer:
M1= 10^-pH, 0.0001 V1= 10.0 mL, 0.01L V2= 1.0L (M1V1=M2V2) => (0.0001M)(0.01L)=M2(1.0L)
Find M2 (Molarity of second solution). This is [H+] M2 aka [H+]= 0.000001 Plug in to this formula to
find pH: pH=-log(H+)
Question:
When 10.0 mL of 0.15 M Na2SO4 solution are diluted to 50.0 mL, what is the final concentration of
sodium ion?
Answer:
Answer: 0.060M
Question:
Explanation
Answer:
M1=0.15 V1=0.01L, V2=0.05L (M1V1=M2V2)=> (0.15M)(0.01L)=M2(0.05L) Find M2 (Molarity of
second solution). This is [H+] M2 aka [H+]=0.030 M Multiply [H+]by number of moles of sodium (2)
(0.030M)(2 moles Na) = 0.060 Concentration of Na
Question:
What is the pH of 15.0 mL of a 0.00345 M solution of CsNO3?
Answer:
Answer: 7.00
Question:
How many mL of 0.40 M HCl are needed to neutralize a liter of 0.0020 M NaOH?
Answer:
Answer: 5.0 mL
Updated Study Material 2026
Question:
Which of the following are weak electrolytes? HCl HC2H3O2 NH3 KCl CH3OH
Answer:
Answers: HC2H3O2 & NH3
Question:
Explanation
Answer:
Weak acids and bases
Question:
A solution has a pH of 4.0. If a second solution has a pH of 8.0, what is the ratio of hydrogen ion ion
concentration in solution 1 compared to solution 2?
Answer:
Answer: 10,000
Question:
What is the hydroxide ion concentration in a solution with a pH of 6.0?
Answer:
Answer: 1.0 x 10^-8 M
Question:
Explanation
Answer:
We know the pH of the solution is 6.0 We can find OH from this formula: OH- = 14- pH Plug in pH to
find hydroxide ion concentration: OH- = 14-6 = 8 So, 1.0 x 10^-8 M
Question:
Which of the following weak acid dissociation constants would result in the least ionization?
Answer:
Answer: Ka = 1.0 x 10^-5
, Question:
If 10.0 mL of an HBr solution with a pH of 4 is diluted to a total volume of 1.0 L what is the pH of the 1
L solution?
Answer:
Answer: 6.0
Question:
Explanation
Answer:
M1= 10^-pH, 0.0001 V1= 10.0 mL, 0.01L V2= 1.0L (M1V1=M2V2) => (0.0001M)(0.01L)=M2(1.0L)
Find M2 (Molarity of second solution). This is [H+] M2 aka [H+]= 0.000001 Plug in to this formula to
find pH: pH=-log(H+)
Question:
When 10.0 mL of 0.15 M Na2SO4 solution are diluted to 50.0 mL, what is the final concentration of
sodium ion?
Answer:
Answer: 0.060M
Question:
Explanation
Answer:
M1=0.15 V1=0.01L, V2=0.05L (M1V1=M2V2)=> (0.15M)(0.01L)=M2(0.05L) Find M2 (Molarity of
second solution). This is [H+] M2 aka [H+]=0.030 M Multiply [H+]by number of moles of sodium (2)
(0.030M)(2 moles Na) = 0.060 Concentration of Na
Question:
What is the pH of 15.0 mL of a 0.00345 M solution of CsNO3?
Answer:
Answer: 7.00
Question:
How many mL of 0.40 M HCl are needed to neutralize a liter of 0.0020 M NaOH?
Answer:
Answer: 5.0 mL
