638 Answered Questions for the topic AP chemistry
Ap Chemistry
04/12/18
If the rate law of a chemical reaction is k[NH4+]2[NO2–], what is the order of the reaction?
I am unsure about whether or not the 2 is the order or the 1.
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For which salt in each of the following groups will the solubility depend on pH
A. AgF, AgCl, AgBr
B. Pb (OH) 2, PbCl2
C. Sr (NO3) 2, Sr (NO2)
D. Ni (NO3) 2, Ni (CN) 2
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Calculate the solubility of the solid Pb3 (PO4) 2 Ksp=1×10^-54 in a 0.10M Pb (NO3) 2
Calculate the solubility of the solid Pb3 (PO4) 2 Ksp=1×10^-54 in a 0.10M Pb (NO3) 2
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Calculate the solubility of Ce (IO3) 3 in a 0.20M KIO3 solution 4.4×10^-8 mol/L Calculate Ksp for Ce (IO3) 3
Calculate the solubility of Ce (IO3) 3 in a 0.20M KIO3 solution 4.4×10^-8 mol/L Calculate Ksp for Ce (IO3) 3
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The Ksp for lead iodide PbI2 is 1.4×10^-8 Calculate the solubility of lead iodide in each of the following
A. Water
B. 0.10M Pb (NO3) 2
C. 0.010M NaI
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The Ksp for silver sulfate (AgSO4) is 1.2×10^-5. Calculate the solubility of silver sulfate in each of the following
A. Water
B. 0.10M Pb (NO3) 2
C. NaI
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Calculate the solubility of Co(OH) 3 Ksp=2.2×10^16 in a buffered solution with a pH=11.0
Calculate the solubility of Co(OH) 3 Ksp=2.2×10^16 in a buffered solution with a pH=11.0
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Calculate the solubility in moles per liter of Fe (OH) 3 Ksp=4×10^-38 in each of the following
A. Water
B. A solution buffered at pH=5.0
C. A solution buffered at pH=11.0
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How do I solve a chemistry problem like this?
C. The density of the concentrated nitric acid used in this experiment was determined to be 1.42 grams per milliliter. Determine the percentage by weight of HNO3 in the original sample of...
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How do I solve this AP Chemistry problem?
B. A 10.00mL sample of the concentrated nitric acid was diluted with water to a total volume of 500.00mL. Then 25.00mL of the diluted acid was tritrated with the standardized NaOH solution prepared...
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Can you please help me with this problem?
The percentage by weight of nitric acid HNO3 in a sample of concentrated nitric acid is to be determined. A. Initially a NaOH solution was standardized by titration with a sample of potassium...
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How do I solve this AP Chemistry problem on H2SO4?
Concentrated sulfuric acid (18.4M H2SO4) has a density of 1.84 grams per millimeter. After dilution with water to 5.20M, the solution has a density of 1.30 grams per milliliter and can be used as...
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How do I solve this AP Chemistry problem on HNO3?
The percentage by weight of nitric acid HNO3 in a sample of concentrated nitric acid is to be determined.
A. Initially a NaOH solution was standardized by titration with a sample of potassium...
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What is the value of the base hydrolysis constant for NaNO2 Ka= 4.5×10^-4
A. 4.5×10^-4
B. 2.2×10^-11
C. 4.5×10^-18
D. 4.5×10^10
E. 2.1×10^-9
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What is the pH of 0.35M KOBr solution? For HOBr Ka=2.5×10^-9
A. 8.60
B. 9.06
C. 11.07
D 11.53
E. 13.54
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What is the value of the base hydrolysis constant for NaNO2, sodium nitrite? Ka=4.5×10^-4 for HNO2
A. 4.5×10^-4
B. 2.2×10^-11
C. 4.5×10^-18
D. 4.5×10^10
E. 2.1×10^-9
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What is the pH of 0.10M sodium acetate (NaAc) solution? The Ka of acetic acid (HAc) is 1.8×10^-5
A. 1.0
B. 0.10
C. 7.0
D. 8.
E. 5.1
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The Ka of the weak acid HNO2 is 7.4×10^4. What is the Kb of its conjugate base NO2-?
The Ka of the weak acid HNO2 is 7.4×10^4. What is the Kb of its conjugate base NO2-?
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Which salt dissolved in water will give the highest pH?
A. NaCl
B. KBr
C. NaNO3
D. NH4Cl
E. NaF
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How many grams of solid sodium acetate should be added to 1.50L of a 0.287M acetic acid solution to prepare a buffer with pH 4.140? Grams sodium acetate=
A. 2.43g
B. 8.77
C. 4.14
D. 8.00
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What is the pH at the equivalence point in the titration of 50.0ml of 0.100M hydrochloric acid HF (Ka=7.2×10^-4) with 0.100M NaOH?
A. 5.88
B. 6.08
C. 7.92
D. 8.12
E. 8.56
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What is the [H3O+] of a solution that is 0.0100M in HOCl ( Ka=3.5×10^-8) and 0.0300M in NaOCl?
A. 2.14×10^-7M
B. 1.45×10^-7M
C. 7.41×10^-8M
D. 2.29×10^-8M
E. 1.17×10^-8M
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Which of the following solutions are good buffer systems?
I. 0.20M calcium hydroxide+0.20M calcium chloride
II. 0.35M+0.32M ammonium nitrate
III. 0.10M hypochlorus acid+0.14M hydrobromic acid
IV. 0.33M barium iodide+0.27M sodium...
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A solution is initially 0.100M in HOCl and 0.300M in NaOCl. What is the pH if 0.030 mol of solid NaOH is added to 1.00L of this solution?
The problem says to assume no change in volume.
The answers are
A. 5.24
B. 5.38
C. 8.02
D. 8.13
E. 9.06
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How do I solve this pH problem on NaOH
If 0.040 moles of solid NaOH is added to 1.0L of a solution that is 0.10M in NH3, and 0.20M in NH4CL, what will be the oH of the resulting solution.
A. 4.80
B. 8.95
C. 5.05
D. 8.65
E. 9.20
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