S20 Ch17 Sec5-6 17 Multiple Choice Question 39 Part A Determine the [H3O+] concentration for a 0.200 M solution of HCI. 4.00 x 10-1 M 1.00 x 10-1 M 1.25 x 1014 M 2.50 x 10-14 M 2.00 x 101 M Submit Request Answer Provide Feedback
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- Calculate the Ka of a 0.500 M acid solution with [H3O+]= 1.7x 10-4M Group of answer choices 1.70 x 10-6 1.5 x 10-1 5.78 x 10-8 5.78 x 10-6 1.5 x 10-7 1.70 x 10-45.20e-03 M solution of a weak base has a pH of 9.60. Calculate the value of pKb for the substance. 5.26 2.94 1.88 The answer is not shown. 6.51Calculate the Ka of a 0.10M acid solution which is 8.1% ionized Group of answer choices 7.1 x 10-5 7.5 x 10-4 8.1 x 10-4 7.1 x 10-4 8.1 x 10-5 8.5 x 10-4
- 1. Calculate the [H 3 O^ + ] solution of 0.075 M HNO 2 and 0.030 M NaNO 2 . The acid dissociation constant, Ka , is 4.5 * 10 ^ - 5 Express your answer in scientific notation as two significant digits (hint: Henderson-Hasselbach). HNO 2(sq) +H 2 O (l) rightleftharpoons H 3 O oop ^ + +NO 2 (ap)ASAP! UPVOTE WILL BE GIVEN! PLEASE WRITE THE SOLUTIONS LEGIBLY. THANK YOU! ANSWER IN 3 DECIMAL PLACES. CHEMISTRY! NO LONG EXPLANATION NEEDED. A 10 ml of concentrated acetic acid was added in a sufficient quantity of water to make 350 ml of the acid solution. SG acetic acid = 1.05 kb acetate = 5.556x10-10 Probable atomic weights: C = 12; H = 1; O = 16; Na = 23 What is the Hydronium ion concentration?please help me answer all 4 a. In the laboratory a student measures the percent ionization of a 0.537 M solution of formic acid , HCOOH to be 1.89 %. Calculate value of Ka =_______ from this experimental data. b. Calculate the percent ionization of a 0.580 M solution of hypochlorous acid. % Ionization = _______ c. In the laboratory, a general chemistry student measured the pH of a 0.537 M aqueous solution of trimethylamine, (CH3)3N to be 11.781. Use the information she obtained to determine the Kb for this base. Kb(experiment) =____________ d. In the laboratory, a general chemistry student measured the pH of a 0.586 M aqueous solution of triethanolamine, C6H15O3N to be 10.780. Use the information she obtained to determine the Kb for this base. Kb(experiment) = ________________
- Calculate the pH of a 0.055 M solution of CH3COONa. (Ka(CH3COOH) = 1.8 x 10-5) Kw= 1.0 x 10-14 Group of answer choices 12.74 4.74 8.74 9.26 5.261. Utilize the following normal values to determine the primary acid-base imbalance and compensation status. (No compensation, partial compensation, complete compensation). Write out at least one cause for each. "A patient that ..." or "A patient has..." Part A: pH=7.32 pCO2=42 mm Hg [HCO3]= 20 mEq/L Cause: Part B: pH=7.55 pCO2=21 mm Hg [HCO3]= 18 mEq/L Cause: Part C: pH=7.26 pCO2=60 mm Hg [HCO3]= 26 mEq/L Cause: Part D: pH=7.56 pCO2=52 mm Hg [HCO3]= 44 mEq/L Cause:Trial 1: Initial pH= 3.92mL Mass of KHP and Paper= 0.868g Mass of paper= 0.357g Mass of KHP= 0.511g Trial 2: Initial pH= 4.09ml Mass of KHP and Paper= 0.870g Mass of paper= 0.359g Mass of KHP= 0.511g 1)Use Kb, the number of moles of C8H4O4^2- at the equivalence point, and the total volume at that point to calculate the pH for each sample at the equivalence point. Compare these calculated results with the experimental results.
- Taking into account the effect of activity, calculate the pH of each of the following: 1. 0.10 M HCL 2. 0.10 M (CH3)2NH2Cl (Ka = 3.2x10-10 for (CH3)2NH2) 3. 0.10 M HCN (Ka = 6.2 x 10-10 for HCN) 4. 0.10 M NaC4H3O5 (for C4H4O5, Ka1 = 2.8 x 10-3, Ka2 = 4.3 x 10-5)Calculate the concentration of A when chemical AB is dissolved in pure water. Ksp = 0.00001331 AB2(s) ⇌ A2+(aq) + 2B¯(aq) Enter answer to 3 sig figs using exponential format.Calculate the pH of a 100-mL solution containing 1.00 g of imidazole (FM 68.08) and 1.00 g of imidazole hydrochloride (FM 104.54).