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Weak acids are weak electrolytes that don’t completely ionize but instead reach a state of equilibrium. What is the percent hydrolysis in 0.075 M sodium acetate, NaCH3COO, solution? When methylammonium chloride is dissolved in water, the reaction that occurs is ____, resulting in a solution that is ____. (ie. The x represents concentration ionized. The hydrated Fe3+ ion is [Fe(OH2)6]3+. b. C6H5OH(aq) + H2O(l) C6H5O-(aq) + H3O+(aq). A 0.10 M solution of which of the following would be most basic? HCO2H. This is a(n) ____ salt. Which electrolyte is not correctly matched? The value of Kb for methylamine, (CH3)2NH, is 7.4 × 10−4. What is the value of the ionization constant for the acid? Which one? A 0.10 M solution of which of the following salts is most acidic? Strong base and weak acid 2HNO2 (aq) + Ba(OH)2 → Ba(NO2) 2 (aq) + 2H2O(l) Assume 25°C. What is the identity of the weak base? The pH of a 0.10 M solution of a monoprotic acid is 2.85. The chief was seen coughing and not wearing a mask. Which of the following salts are incorrectly matched with its description? What is the concentration of H3O+ ions in a solution in which pH = 4.32? Calculate the [OH−] in 0.050 M potassium fluoride, KF. What is the pH of 500. mL of solution containing 0.0124 gram of Ca(OH)2? What is the experimentally determined value of Ka for HClO3? What is the concentration of A3− ions at equilibrium for a 0.10 M solution of a hypothetical triprotic acid H3A, with Ka1 = 6.0 × 10−3, Ka2 = 2.0 × 10−8, and Ka3 = 1.0 × 10−14? double displasment, single displacement, neutralize)? The hypothetical weak acid H2A ionizes as shown below. HCl. A solution having a pH of 1.4 would be described as ____. You can sign in to vote the answer. Which one of the following is an insoluble base? Calculate the ionization constant for a weak acid, HA, that is 1.60% ionized in 0.0950 M solution. Each response gives a pair of solutions. The [OH−] = 1.3 × 10−6 M for a 0.025 M solution of a weak base. In a solution containing only a weak monoprotic acid HA, [H3O+] is ____ [A−]; if the solution is not very dilute, the concentration of nonionized HA is approximately equal to the ____ of the solution. We make a 1.0 M solution of an unknown acid, HX. What is the percent hydrolysis of Fe2+ in a 0.30 M FeCl2 solution? … Which of the following is a soluble, strong base? HF is weak the rest are strong acids and electrolytes. Which of the equations below illustrates this reaction for phenol? Calculate the (base) hydrolysis constant for the hypochlorite ion, OCl−. The hydronium ion concentration in an aqueous solution at 25oC is 6.1 x 10-2M. e. 0.010 M (COOH)2 Ka1 = 5.9 × 10−2, Ka2 = 6.4 × 10−5. The reaction that occurs when NH4Br dissolves in water is ____. d.all are strong acids and HF is one of the most dangerous. Ka = 3.5 × 10−8, Calculate the value of [H3O+] in a 0.010 M HOBr solution. What is the value of Ka for this acid? d. HX is a weak acid with a Ka value of about 10−10. Ka = 2.5 × 10−9, Calculate the pH of 0.10 M HCN solution. The pH of a solution of hydrochloric acid is 2.80. Should I call the police on then? The pH of a solution of Ba(OH)2 is 9.40. Which pH or pOH value is incorrectly matched with its description? What is the hydroxide ion concentration in this solution? Consider an aqueous solution of ammonium hypochlorite. The pH of a weak monoprotic acid (HA) is 3.75. What is the pH of a 0.400 M HNO3 solution? rt A Which of the following is a WEAK acid? What is the molarity of the acid? Which one of the following salts is insoluble in water? Ka = 4.5 × 10−4 for HNO2. Which one is always true? Which of the following has the strongest conjugate base? What is the pH of 0.15 M solution of trimethylammonium nitrate, (CH3)3NHNO3, a salt? With a pH meter, we determine that the pH of the solution is 5.00. Which one of the following is a soluble strong electrolyte? The hydrated ferrous ion is [Fe(OH2)6]2+. Which of the following acid / base pairs produce neutral salts when they react? Evaluate the (base) hydrolysis constant for sodium cyanate, NaOCN. A solution in which the pOH is 12.5 would be described as ____. What is the pH of a solution which has a hydroxide ion concentration of 2.5 x 10-2M? Consider a solution that is 0.10 M in a weak triprotic acid that is represented by the general formula H3A with the following ionization constants. What is the molarity of this solution of base? A 0.010 M aqueous solution of a weak acid HA has a pH of 5.0. The pH of a 0.20 M solution of a weak monoprotic acid is 3.70. Calculate the pKa for a weak acid, HA, that is 2.3% ionized in 0.080 M solution? Calculate the pH of 0.050 M Ba(CN)2 solution. What is the [OH−] in 0.20 M sodium cyanate, NaOCN, solution? c. The ionizations of polyprotic acids occur simultaneously. d. According to Brønsted-Lowry the anions of strong acids are very strong bases. Which one could not possibly have the pH designated? Which of the following statements about measurement of pH is incorrect? Which of the following statements about the HX is true? Consider the reaction NH3(aq) + H2O(l) NH4+(aq) + OH-(aq). Calculate the value of Kb for this weak base. Consider calculations of [H3O+] in each of the following solutions. H2SO4. While technically a weak acid, hydrofluoric acid is extremely powerful and highly corrosive. Calculate the acid ionization constant of an unknown monoprotic weak acid, HA, if its salt, NaA, has a (base) hydrolysis constant of 6.2 × 10−9. Calculate the pH of 0.10 M solution of NaBO2. Which one of the following salts produces acidic solutions when it is dissolved in water? The pH of a 0.100 M solution of a weak acid, HA, is 3.50. What is the value of the (base) hydrolysis constant for NaNO2, sodium nitrite? Calculate the [H3O+] in 0.030 M potassium fluoride, KF. The percent ionization of a 0.331M solution of HCN is found to be 0.00337%. When sodium benzoate is dissolved in water, the reaction that occurs is ____, resulting in a solution that is ____. What is the pH of a 0.10 M CuCl2 solution? Which one of the following salts produces basic solutions when it is dissolved in water? How do you think about the answers? When salts derived from ____ acids and ____ bases are dissolved in water, the resulting solution is always acidic. Calculate the percent hydrolysis of the hypochlorite ion in 0.10 M NaOCl solution. Calculate the [HA−] in 0.20 M H2A. Which one of the following substances is not a strong electrolyte? Which of the following statements about polyprotic acids is incorrect? what type of reaction is Na2B4O7.10H2O + 2HCl -> 2NaCl(aq) + 5H2O + 4B(OH)3. A 0.10 M solution of which of the following salts is neutral? The Ka values for weak acids are equal to the pH for dilute solutions. Calculate the pH of a 0.308 M ascorbic acid solution, H2C6H6O6 (aq). Calculate the pKa for this acid. Ka = 6.3 × 10−5, What is the [OH−] in a 0.25 M hypobromous acid (HOBr) solution? Ka = 1.8 × 10−5. b. Ka for formic acid (HCOOH) is 1.8 x 10-4. What is the pH of 0.51 M Ca(CH3COO)2 solution? Do not go through the calculations. Ka = 4.5 × 10−4, Calculate the pH of a solution of acetic acid that is 3.0% ionized. Calculate the pH of a 0.050 M Fe(NO3)3 solution. Join Yahoo Answers and get 100 points today. For which calculation is it not reasonable to assume that "x" is much less than the initial concentration? Which of the following relationships in incorrect? Which response includes all the following salts that give acidic aqueous solutions, and no other salts? The hydrated beryllium ion is [Be(OH2)4]2+. What is the pH of a 1.0L solution of 0.445 M hydrocyanic acid, HCN? Calculate the pH of 3.2 × 10−3 M H2CO3 solution. (CH3)NH3+ + H2O (CH3)NH2 + H3O+; acidic. When solid NH4NO3 is added to water, the pH ____. Kb = 1.8 × 10−5, Calculate the value of [H3O+] in a 0.18 M solution of aqueous aniline. Calculate the percent ionization of the acid in 0.100 M solution. The pH of a solution is −0.38. Ka = 4.0 × 10−10, Calculate the pH of 0.050 M benzoic acid solution. Ka = 1.8 × 10−5, How many moles of nitrous acid, HNO2, are required initially to prepare 2.5 liters of a solution of pH = 3.00? Which of the following salts produce acidic solutions? What is Ka for the NH4+ ion at 25°C? b. What is the equilibrium constant for the following reaction: What is the pH of an aqueous solution of 0.184M carbonic acid, H2CO3? b. salt / cation of an acid, anion of a base. Which solution would have the lowest [OH−]? What is the hydrogen ion concentration in a solution having a pOH of 3.62? The only weak acid formed by the reaction between hydrogen and a halogen is hydrofluoric acid (HF). A 0.100 M solution of this acid has [H3O+] = 0.0070 M. What is the value of Ka for Cl2HCCOOH? What is the pH of this solution? The [H3O+] = 2.0 × 10−4 M for a 0.020 M solution of a weak acid. Of the following, which acids are weak acids? Aqueous solutions of one of the following is acidic. Dichloroacetic acid is a weak monoprotic acid. Which one of the following is a weak acid? Which response lists the species present in the highest concentration in a solution of 0.20 M H3PO4? What is the degree of ionization of HA in the solution? What is the hydronium-ion concentration of a 0.0029 M KOH solution? Which salt is produced from a strong acid and a strong base? 5.5 M HF c. 0.095 M H2SO4 d. None are weak acids, all are strong acids.

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