chemistry 2 ,50 questions

Determine the pH in a 0.667 M NaOH solution.Group of answer choices0.120.1814.1813.8813.82Question 22 ptsWhat 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 choices3.9414.0910.243.765.48Question 32 ptsDetermine the pH of a 0.22 M NaF solution at 25°C. The Ka of HF is 3.5 × 10-5.Group of answer choices5.1011.4410.208.902.56Question 42 ptsWhich of the following compounds solubility will NOT be affected by a low pH in solution?Group of answer choicesBaCO3AgClCuSMg(OH)2BaF2Question 52 ptsDetermine 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 M4.0 × 10-4 M0.30 M1.4 × 10-6 M4.9 × 10-3 MQuestion 62 ptsCalculate the pH for an aqueous solution of pyridine that contains hydroxide ion.Group of answer choices4.15 × 10-47.052.41 × 10-1110.623.38Question 72 ptsIdentify the base that is in baking soda.Group of answer choicesNaHCO3LiOHKHCO3RbOHLi2CO3Question 82 ptsA 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 choices8.8511.829.187.104.82Question 92 ptsDetermine the [H3O+] concentration for a 0.200 M solution of HCl.Group of answer choices1.00 × 10-1 M4.00 × 10-1 M2.50 × 10 -14 M1.25 × 10-14 M2.00 × 10-1 MFlag question: Question 10Question 102 ptsA ligand is a molecule or ion that acts as aGroup of answer choicesLewis base.Brønsted-Lowry base.conjugate acid.Arrhenius base.Lewis acid.Flag question: Question 11Question 112 ptsCalculate 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 choices10.635.0733.36914.384.121Flag question: Question 12Question 122 ptsA 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 choices1.520.682.3512.483.22Flag question: Question 13Question 132 ptsWhat is the pH of a 0.020 M Ba(OH)2 solution?Group of answer choices1.701.4012.6013.2012.30Flag question: Question 14Question 142 ptsA 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)2CdSNH4ClFeSAgClFlag question: Question 15Question 152 ptsWhich of the following is a Lewis acid?Group of answer choicesAlBr3CHBr3NH3CCl4None of the above is a Lewis acid.Flag question: Question 16Question 162 ptsCalculate 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 × 10-65.50 × 10-118.07 × 10-37.18 × 10-15.25 × 10-7Flag question: Question 17Question 172 ptsWhat 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 M1.9 × 10-5 M1.9 × 10-4 M5.9 × 10-5 MFlag question: Question 18Question 182 ptsWhat 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 choices7.005.286.2210.028.72Flag question: Question 19Question 192 ptsCalculate 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 choices6.465.997.067.548.01Flag question: Question 20Question 202 ptsCalculate 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 choices3.5810.256.370.80Flag question: Question 21Question 212 ptsWhat is the hydroxide ion concentration of a NaOH solution that has a pH of 12.20?Group of answer choices12.20 M1.58 × 10-2 M1.80 M7.206.31 × 10-13 MFlag question: Question 22Question 222 ptsCalculate 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 choices3.60710.914.55414.263.093Flag question: Question 23Question 232 ptsWhat 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 CH3CO2HGroup of answer choices6.625.299.804.208.71Flag question: Question 24Question 242 ptsPlace the following in order ofincreasingacid strength.HBrO2HBrO3HBrOHBrO4Group of answer choicesHBrO4 < HBrO2 < HBrO3 < HBrOHBrO < HBrO4 < HBrO3 < HBrO2HBrO2 < HBrO4 < HBrO < HBrO3HBrO < HBrO2 < HBrO3 < HBrO4HBrO2 < HBrO3 < HBrO4 < HBrOFlag question: Question 25Question 252 ptsDetermine the pH of a 0.00444 M HClO4 solution.Group of answer choices1.3532.35312.64711.6475.824Flag question: Question 26Question 262 ptsA 6.0 × 10-3 M aqueous solution of Ca(OH)2 at 25.0°C has a pH of ________.Group of answer choices5.6 × 10-1312.081.9211.781.2 × 10-2Flag question: Question 27Question 272 ptsAn aqueous solution at 25.0°C contains [H+] = 0.099 M. What is the pH of the solution?Group of answer choices0.09901.0013.0-1.001.20 × 10-13Flag question: Question 28Question 282 ptsCalculate the molar solubility of thallium chloride in 0.0.25 M NaCl at 25°C. Ksp for TlCl isGroup of answer choices8.2 × 10-3 M6.8 × 10-4 M1.7 × 10-5 M1.3 × 10-2 MFlag question: Question 29Question 292 ptsCalculate the pH for an aqueous hydroiodic acid solution that contains hydronium ion.Group of answer choices11.502.5012.503.17 × 10-123.15 × 10-3Flag question: Question 30Question 302 ptsDescribe what happens at high pH for aluminum hydroxide.Group of answer choicesAl(H2O)23+ precipitates.Al precipitates.Al dissolves.Al(H2O)2(OH)4- dissolves.Al(OH)5 precipitates.Flag question: Question 31Question 312 ptsWhich 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 × 10-2HIO, Ka = 2.3 × 10-10HCN, Ka = 4.9 × 10-10C6H5OH, Ka = 1.3 × 10-10HN3, Ka = 2.5 × 10-5Flag question: Question 32Question 322 ptsHow many milliliters of 0.0991 M LiOH are required to titrate 25.0 mL of to the equivalence point?Group of answer choices0.2084.5829.521.20.333Flag question: Question 33Question 332 ptsA solution contains Ba2+, Hg2+, Ag+, NH4+, and Fe2+. Identify the precipitate after the addition of 6 M HCl.Group of answer choicesHgSBa3(PO4)2FeSAgClNH4ClFlag question: Question 34Question 342 ptsIdentify the diprotic acid.Group of answer choicesCH3COOHHNO3H2SO3HClO4HFFlag question: Question 35Question 352 ptsFind 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%3.2%1.1%3.5 × 10-2%Flag question: Question 36Question 362 ptsIdentify theweakmonoprotic acid.Group of answer choicesH2CO3NaBrHFHNO3LiOHFlag question: Question 37Question 372 ptsDetermine the pH of a 0.141 M RbOH solution at 25°C.Group of answer choices13.8613.150.1410.8510.88Flag question: Question 38Question 382 ptsCalculate the pH of a solution that contains 7.8 × 10-6 M OH? at 25°C.Group of answer choices8.8912.721.285.119.64Flag question: Question 39Question 392 ptsWhat 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 choices10.892.1111.376.222.63Flag question: Question 40Question 402 ptsA 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 choices1.211.120.862.002.86Flag question: Question 41Question 412 ptsFormic 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 M0.0375 M0.0190 M0.0567 M0.0134 MFlag question: Question 42Question 422 ptsWhich 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 = 4.19HF, pKa = 3.46HClO, pKa = 7.54H2SO3, pKa = 1.77HClO2, pKa = 1.96Flag question: Question 43Question 432 ptsCalculate 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 choices7.466.677.747.546.34Flag question: Question 44Question 442 ptsA 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 choices1.3512.8512.6513.130.87Flag question: Question 45Question 452 ptsCalculate 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 choices4.862.063.563.763.16Flag question: Question 46Question 462 ptsWhich one of the following salts, when dissolved in water, produces the solution with thehighestpH?Group of answer choicesCsClCsICsFCsBrFlag question: Question 47Question 472 ptsWhat 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 choices2.100.403.233.764.08Flag question: Question 48Question 482 ptsA 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)2ZnSNH4BrAgClHgSFlag question: Question 49Question 492 ptsA 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 choices3.468.147.009.6210.54Flag question: Question 50Question 502 ptsThelargestchange in pH for an effective buffer occurs when the base is how many times as concentrated as the acid?Group of answer choices62054010