chemistry 2 ,50 questionsrachelcerr
Determine the pH in a 0.667 M NaOH solution.
Group of answer choices0.12
Question 22 pts
What is the pH of a buffer solution that is 0.192 M in lactic acid and 0.155 M in sodium lactate? The Ka of lactic acid is 1.4 × 10-4.
Group of answer choices3.94
Question 32 pts
Determine the pH of a 0.22 M NaF solution at 25°C. The Ka of HF is 3.5 × 10-5.
Group of answer choices5.10
Question 42 pts
Which of the following compounds solubility will NOT be affected by a low pH in solution?
Group of answer choicesBaCO3
Question 52 pts
Determine the molar solubility of CaSO4 in a solution containing 0.060 M Na2SO4. Ksp (CaSO4) = 2.4 × 10-5.
Group of answer choices5.8 × 10-10 M
4.0 × 10-4 M
1.4 × 10-6 M
4.9 × 10-3 M
Question 62 pts
Calculate the pH for an aqueous solution of pyridine that contains hydroxide ion.
Group of answer choices4.15 × 10-4
2.41 × 10-11
Question 72 pts
Identify the base that is in baking soda.
Group of answer choicesNaHCO3
Question 82 pts
A 25.0 mL sample of 0.150 M butanoic acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The Ka of butanoic acid is 1.5 × 10-5.
Group of answer choices8.85
Question 92 pts
Determine the [H3O+] concentration for a 0.200 M solution of HCl.
Group of answer choices1.00 × 10-1 M
4.00 × 10-1 M
2.50 × 10 -14 M
1.25 × 10-14 M
2.00 × 10-1 M
Flag question: Question 10Question 102 pts
A ligand is a molecule or ion that acts as a
Group of answer choicesLewis base.
Flag question: Question 11Question 112 pts
Calculate the pH of a solution that is 0.112 M in sodium formate (NaHCO2) and in formic acid The Ka of formic acid is 1.77 × 10-4.
Group of answer choices10.63
Flag question: Question 12Question 122 pts
A 700.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M CsOH. Determine the pH of the solution after the addition of 350.0 mL of CsOH.
Group of answer choices1.52
Flag question: Question 13Question 132 pts
What is the pH of a 0.020 M Ba(OH)2 solution?
Group of answer choices1.70
Flag question: Question 14Question 142 pts
A solution contains Fe2+, Ba2+, Ag+, NH4+, and Cd2+. Identify the soluble compound after the addition of 6 M HCl; then H2S and 0.2 M HCl; then OH- to a pH of 8; and then (NH4)2HPO4 with NH3.
Group of answer choicesBa3(PO4)2
Flag question: Question 15Question 152 pts
Which of the following is a Lewis acid?
Group of answer choicesAlBr3
None of the above is a Lewis acid.
Flag question: Question 16Question 162 pts
Calculate the Ksp for hydroxide if the solubility of Mn(OH)2 in pure water is 7.18 × 10-1 g/L.
Group of answer choices2.10 × 10-6
5.50 × 10-11
8.07 × 10-3
7.18 × 10-1
5.25 × 10-7
Flag question: Question 17Question 172 pts
What is the hydronium ion concentration of a 0.100 M hypochlorous acid solution with The equation for the dissociation of hypochlorous acid is:
HOCl(aq) + H2O(l) ⇌ H3O+(aq) + OCl-(aq)
Group of answer choices5.9 × 10-4 M
1.9 × 10-5 M
1.9 × 10-4 M
5.9 × 10-5 M
Flag question: Question 18Question 182 pts
What is the pH of a solution made by mixing 29.00 mL of 0.10 M acetic acid with 29.00 mL of 0.10 M KOH? Assume that the volumes of the solutions are additive. Ka = for CH3CO2H.
Group of answer choices7.00
Flag question: Question 19Question 192 pts
Calculate the pH of a solution formed by mixing 150.0 mL of 0.20 M HClO with 300.0 mL of 0.30 M CsClO. The Ka for HClO is 2.9 × 10-8.
Group of answer choices6.46
Flag question: Question 20Question 202 pts
Calculate the pH of a 0.16 M carbonic acid solution, H2CO3(aq), that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.
Group of answer choices3.58
Flag question: Question 21Question 212 pts
What is the hydroxide ion concentration of a NaOH solution that has a pH of 12.20?
Group of answer choices12.20 M
1.58 × 10-2 M
6.31 × 10-13 M
Flag question: Question 22Question 222 pts
Calculate the pH of a solution that is 0.322 M in nitrous acid (HNO2) and 0.178 M in potassium nitrite (KNO2). The acid dissociation constant of nitrous acid is 4.50 × 10-4.
Group of answer choices3.607
Flag question: Question 23Question 232 pts
What is the pH of the resulting solution if 45.00 mL of 0.10 M acetic acid is added to 10.00 mL of 0.10 M KOH? Assume that the volumes of the solutions are additive. Ka = 1.8 × 10-5 for CH3CO2H
Group of answer choices6.62
Flag question: Question 24Question 242 pts
Place the following in order of increasing acid strength.
Group of answer choicesHBrO4 < HBrO2 < HBrO3 < HBrO
HBrO < HBrO4 < HBrO3 < HBrO2
HBrO2 < HBrO4 < HBrO < HBrO3
HBrO < HBrO2 < HBrO3 < HBrO4
HBrO2 < HBrO3 < HBrO4 < HBrO
Flag question: Question 25Question 252 pts
Determine the pH of a 0.00444 M HClO4 solution.
Group of answer choices1.353
Flag question: Question 26Question 262 pts
A 6.0 × 10-3 M aqueous solution of Ca(OH)2 at 25.0°C has a pH of ________.
Group of answer choices5.6 × 10-13
1.2 × 10-2
Flag question: Question 27Question 272 pts
An aqueous solution at 25.0°C contains [H+] = 0.099 M. What is the pH of the solution?
Group of answer choices0.0990
1.20 × 10-13
Flag question: Question 28Question 282 pts
Calculate the molar solubility of thallium chloride in 0.0.25 M NaCl at 25°C. Ksp for TlCl is
Group of answer choices8.2 × 10-3 M
6.8 × 10-4 M
1.7 × 10-5 M
1.3 × 10-2 M
Flag question: Question 29Question 292 pts
Calculate the pH for an aqueous hydroiodic acid solution that contains hydronium ion.
Group of answer choices11.50
3.17 × 10-12
3.15 × 10-3
Flag question: Question 30Question 302 pts
Describe what happens at high pH for aluminum hydroxide.
Group of answer choicesAl(H2O)23+ precipitates.
Flag question: Question 31Question 312 pts
Which of the following acids (listed with Ka values) and their conjugate base should be used to form a buffer with a pH of 2.34?
Group of answer choicesHClO2, Ka = 1.1 × 10-2
HIO, Ka = 2.3 × 10-10
HCN, Ka = 4.9 × 10-10
C6H5OH, Ka = 1.3 × 10-10
HN3, Ka = 2.5 × 10-5
Flag question: Question 32Question 322 pts
How many milliliters of 0.0991 M LiOH are required to titrate 25.0 mL of to the equivalence point?
Group of answer choices0.208
Flag question: Question 33Question 332 pts
A solution contains Ba2+, Hg2+, Ag+, NH4+, and Fe2+. Identify the precipitate after the addition of 6 M HCl.
Group of answer choicesHgS
Flag question: Question 34Question 342 pts
Identify the diprotic acid.
Group of answer choicesCH3COOH
Flag question: Question 35Question 352 pts
Find the percent ionization of a 0.337 M HF solution. The Ka for HF is 3.5 × 10-4.
Group of answer choices4.7%
1.2 × 10-2%
3.5 × 10-2%
Flag question: Question 36Question 362 pts
Identify the weak monoprotic acid.
Group of answer choicesH2CO3
Flag question: Question 37Question 372 pts
Determine the pH of a 0.141 M RbOH solution at 25°C.
Group of answer choices13.86
Flag question: Question 38Question 382 pts
Calculate the pH of a solution that contains 7.8 × 10-6 M OH⁻ at 25°C.
Group of answer choices8.89
Flag question: Question 39Question 392 pts
What is the pH of a 0.300 M NH3 solution that has Kb = 1.8 × 10-5? The equation for the dissociation of NH3 is:
NH3(aq) + H2O(l) ⇌ NH4+(aq) + OH-(aq)
Group of answer choices10.89
Flag question: Question 40Question 402 pts
A 150.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH. Determine the pH of the solution after the addition of 45.0 mL of LiOH.
Group of answer choices1.21
Flag question: Question 41Question 412 pts
Formic acid (HCO2H, Ka = 1.8 × 10-4) is the principal component in the venom of stinging ants. What is the molarity of a formic acid solution if 25.00 mL of the formic acid solution requires 74.80 mL of 0.0567 M NaOH to reach the equivalence point?
Group of answer choices0.170 M
Flag question: Question 42Question 422 pts
Which of the following acids (listed with pKa values) and their conjugate base should be used to form a buffer with a pH of 8.10?
Group of answer choicesHC7H5O2, pKa = 4.19
HF, pKa = 3.46
HClO, pKa = 7.54
H2SO3, pKa = 1.77
HClO2, pKa = 1.96
Flag question: Question 43Question 432 pts
Calculate the pH of a buffer that is 1.26 M HClO and 0.079 M NaClO. The Ka for HClO is 2.9 × 10-8.
Group of answer choices7.46
Flag question: Question 44Question 442 pts
A 550.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M KOH. Determine the pH of the solution after the addition of 550.0 mL of KOH.
Group of answer choices1.35
Flag question: Question 45Question 452 pts
Calculate the pH of a buffer that is 0.080 M HF and 0.040 M NaF. The Ka for HF is 3.5 × 10-4.
Group of answer choices4.86
Flag question: Question 46Question 462 pts
Which one of the following salts, when dissolved in water, produces the solution with the highest pH?
Group of answer choicesCsCl
Flag question: Question 47Question 472 pts
What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.40 M HCl to reach the equivalence point? Ka = 3.0 × 10-8 for HOCl.
Group of answer choices2.10
Flag question: Question 48Question 482 pts
A solution contains Zn2+, Hg2+, Ag+, NH4+, and Ba2+. Identify the precipitate after the addition of 6 M HCl, then H2S and 0.2 M HCl.
Group of answer choicesBa3(PO4)2
Flag question: Question 49Question 492 pts
A 220.0 mL sample of 0.20 M HF is titrated with 0.10 M NaOH. Determine the pH of the solution after the addition of 440.0 mL of NaOH. The Ka of HF is 3.5 × 10-4.
Group of answer choices3.46
Flag question: Question 50Question 502 pts
The largest change in pH for an effective buffer occurs when the base is how many times as concentrated as the acid?
Group of answer choices6
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