Chemistry 51 - Fundamentals of Chemistry » Fall 2021 » Acids and Bases Worksheet
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Question #1
What are the coefficients to balance the following equation? ____ H3PO4 + ____ KOH → _____ K3PO4 + ___ H2O
A.
1,3,1,3
B.
1,1,3,3
C.
3,2,1,1
Question #2
What are the coefficients to balance the following equation? ___ H2SO4 + ___ Al(OH)3 → ___ Al2(SO4)3 + ___ H2O
A.
3,2,1,6
B.
1,3,1,3
C.
3,2,1,1
Question #3
Identify the acid and its conjugate base in the following chemical equation: Na3PO4 + NaHCO3 → Na2CO3 + Na2HPO4 acid = ___________ conjugate base = ____________
A.
Na2CO3, NaHCO3
B.
Na3HCO3, Na3CO2
C.
NaHCO3, Na2CO3
Question #4
Identify the base and its conjugate acid in the following chemical equation: Na2CO3 + H2O → NaHCO3 + NaOH acid = ___________ conjugate base = ____________
A.
Na2CO3, NaHCO3
B.
Na2HCO3, NaH3CO
C.
NaHCO3, Na2CO3
Question #5
Which of the following solutions is the most acidic?
A.
[OH-] = 10-13 M
B.
pH = 3
C.
[H+] = 2 X 10-9 M
D.
[H+] = 10-11 M
Question #6
heat + 3 NO2 ⇌ N2O5 + NO For the chemical system above at equilibrium, if N2O5 is added, Le Chatelier's Principle would predict that the concentration of NO, [NO], would __________.
A.
stay the same
B.
decrease
C.
increase
Question #7
heat + 3 NO2 ⇌ N2O5 + NO For the chemical system above at equilibrium, if N2O5 is added, Le Chatelier's Principle would predict that the temperature would __________.
A.
decrease
B.
increase
C.
stay the same
Question #8
heat + 3 NO2 ⇌ N2O5 + NO For the chemical system above at equilibrium, if N2O5 is added, Le Chatelier's Principle would predict that the concentration of NO2, [NO2], would __________.
A.
decrease
B.
stay the same
C.
increase
Question #9
How many milliequivalents (mEq) are in 0.25 moles of FeCl3? Note: one equivalent (Eq) of charge is equal to one mole of + charge ions. 1 Eq = 1000 mEq.
A.
750
B.
250
C.
500
Question #10
How many moles of CuSO4 are present if a solution is measured to have 400 milliequivalents (mEq)? Note: one equivalent (Eq) of charge is equal to one mole of + charge ions. 1 Eq = 1000 mEq.
A.
1
B.
0.2
C.
5
Question #11
What is the pH of a buffer solution that contains 0.25 M HPO42- and 0.50 M H2PO4-? Round your final answer to two decimal places. pKa of HPO42- is 12.44 pKa of H2PO4- is 7.21 pH = pKa + log10 ( [base] / [acid] )
A.
6.91
B.
7.11
C.
6.11
Question #12
2 H3PO4 + 3 Ba(OH)2 → Ba3(PO4)2 + 6 H2O For the above chemical equation, what is the molarity of a Ba(OH)2 solution if 25.0 mL of it will exactly neutralize 40.0 mL of 0.200 M H3PO4?
A.
0.28
B.
0.48
C.
0.44
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