what is the pK b of a 0.450 M solution of hypoiodous acid, HOI? ( Ka1 = 2.3x10 -
ID: 894257 • Letter: W
Question
what is the pKb of a 0.450 M solution of hypoiodous acid, HOI? ( Ka1 = 2.3x10-11)
a. 10.29 b. 10.64 c. 5.15 d. 3.36 e. 8.85
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a solution is prepared by adding 0.10 mol of potasium acetate, KCH3COO, to 1.00 L of water. which statement about the solution is correct?
a. concentration of acetate ions > than the concentration of potassium ions
b. solution is neutral
c. concentration of potassiuom ions and acetate is identical
d. solution is basic
e. solution is acidic
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what is the pH of a 0.879 M solution of phosphoric acid, H3PO4? Ka1 = 7.5x10-3 Ka2 = 6.2x10-8 Ka3 = 4.8x10-13
a. 3.64 b. 7.28 c. 1.09 d. 2.18 e. 0.06
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what is the pH of a 0.900M solution of canic acid, HOCN? Ka1 = 3.5x10-4
a. 12.2 b. 1.8 c. 3.5 d. 10.5 e. 4.6
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what is the pOH of a 0.050 M HBr solution?
a. 1.30 b. 1.12 c. 12.70 d. 11.00 e. 0.89
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butyric acid is responsible for the odor in rancid butter. A solution of 0.25 M butyric acid has a pH of 2.71. what is the Ka for the acid?
given the equation Ag2CO3(s) <--> 2Ag+(aq)+CO32-(aq). what is the solubility product expression, Ksp, of silver carbonate.
Ksp silver carbonate = 8.4x10-12
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which of the following substances has the greatest solubility in water?
a. ZnCO3 (Ksp=1.2x10-10) b. Ag2CO3 (Ksp=8.4x10-12) c. Cr(OH)3 (Ksp=6.7x10-31) d. AgCl (Ksp= 1.8x10-10) e. Mn(OH)2 (Ksp=2.1x10-13)
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what is the pH of a solution after titrating 50.0 mL of 0.650 pyridine, C5H5N (Kb = 1.8x10-9), with 50.0 mL of HCl?
a. 4.47 b. 2.71 c. 5.74 d. 2.87 e. 5.43
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a 10.0 mL sample of 0.75 M CH3CH2CO2H (ka1=1.3x10-5) is titrated with 0.30 M NaOH. what is the pH of the solution after 22.0 mL of NaOH have been added to the acid?
a. 4.89 b. 5.00 c. 5.75 d. 4.12 e. 2.50
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what is the pH of a solution prepared with 0.50 M HC3H5O3 (lactic acid) (Ka1 = 1.4x10-4) and 0.75 M NaC3H5O3 (sodium lactate)?
a. 0.46 b. 2.00 c. 3.68 d. 4.03 e. 3.85
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calculate the solubility of sliver chromate , Ag2CrO4 (Ksp=1.1x10-12), in 0.005 M Na2CRO4.
a. 3.4x10-5 b. 1.0x10-6 c. 8.2x10-5 d. 5.2x10-7 e. 7.4x10-6
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if the solubility of barium fluoride is 7.2x10-3 M, what is the Ksp of BaF2?
a. 7.5x10-7 b. 3.7x10-7 c. 7.2x10-3 d. 1.5x10-6 e. 5.2x10-5
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which of the following aqueous misxtures would be a buffer system?
a. NH3(Kb=1.8x10-5), NaOH b. H2SO4(Ka1=very large)(Ka2=1.2x10-2), CH3COOH(Ka1=1.8x10-5) c. H3PO4(Ka1=7.5x10^-3)(Ka2=6.2s10^-8)(Ka3=4.8x10^-13), NaH2PO4 d. HCl, NaCl e. HNO3,NaNO3
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How many grams of NaOBr should be added to 50.0 mL of 0.650 M of HOBr(Ka1=2.0x10-9) to make a buffer at pH 8.90
Explanation / Answer
Solutions :-
a solution is prepared by adding 0.10 mol of potasium acetate, KCH3COO, to 1.00 L of water. which statement about the solution is correct?
Solution :- potassium acetate is the conjugate base of the acetic acid therefore when it added to water then it forms the OH- ions
So the solution will be basic in nature
Therefore correct answer is option ‘d’
what is the pH of a 0.879 M solution of phosphoric acid, H3PO4? Ka1 = 7.5x10-3 Ka2 = 6.2x10-8 Ka3 = 4.8x10-13
Solution :- using the ka1 lets calculate the pH
Ka= [H2PO4^-] [H3O+]/[H3PO4]
7.5*10^-3 = [x][x]/[0.879-x]
7.5*10^-3 * 0.879-x = x^2
Solving for x we get
x= 0.0775
therefore pH = -log [H3O+]
= - log [0.0775]
= 1.1
So the correct answer is option ‘c’
what is the pH of a 0.900M solution of canic acid, HOCN? Ka1 = 3.5x10-4
Solution : -
Ka = [ H3O+] [ OCN^-] /[HOCN]
3.5*10^-4= [x][x]/[0.900 –x]
3.5*10^-4 * 0.900-x =x^2
X= 0.0176
pH= -log [H3O+]
pH= -log [0.0176]
pH= 1.8
So the correct answer is option ‘b’
what is the pOH of a 0.050 M HBr solution?
Solution :- HBr is the strong acid
Therefore
pH= -log [H+]
pH= -log [0.050]
pH= 1.30
pH+ pOH = 14
therefore pOH = 14- pH
= 14 -1.30
= 12.70
Therefore the correct answer is option ‘c’
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