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Introductory Chemistry (6th Edition)
- Ionization of the first proton from H2SO4 is complete (H2SO4 is a strong acid); the acid-ionization constant for the second proton is 1.1 102. a What would be the approximate hydronium-ion concentration in 0.100 M H2SO4 if ionization of the second proton were ignored? b The ionization of the second proton must be considered for a more exact answer, however. Calculate the hydronium-ion concentration in 0.100 M H2SO4, accounting for the ionization of both protons.arrow_forwardIonization of the first proton from H2SeO4 is complete (H2SeO4 is a strong acid); the acid-ionization constant for the second proton is 1.2 102. a What would be the approximate hydronium-ion concentration in 0.150 M H2SeO4 if ionization of the second proton were ignored? b The ionization of the second proton must be considered for a more exact answer, however. Calculate the hydronium-ion concentration in 0.150 M H2SeO4, accounting for the ionization of both protons.arrow_forwardWhat is [OH-] in a solution of 1.25 M NH3 and 0.78 M NH4NO3?. NH3(aq)+H2O(l)NH4+(aq)+OH(aq)Kb=1.8105arrow_forward
- Each box represents an acid solution at equilibrium. Squares represent H+ ions. Circles represent anions. (Although the anions have different identities in each figure, they are all represented as circles.) Water molecules are not shown. Assume that all solutions have the same volume. (a) Which figure represents the strongest acid? (b) Which figure represents the acid with the smallest Ka? (c) Which figure represents the acid with the lowest pH?arrow_forwardCalculate [CO32] in a 0.010-M solution of CO2 in water (usually written as H2CO3). If all the CO32 in this solution comes from the reaction HCO3(aq)H+(aq)+CO32(aq) what percentage of the H+ ions in the solution is a result of the dissociation of HCO3? When acid is added to a solution of sodium hydrogen carbonate (NaHCO3), vigorous bubbling occurs. How is this reaction related to the existence of carbonic acid (H2CO3) molecules in aqueous solution?arrow_forwardConsider two separate aqueous solutions: one of a weak acid HA and one of HCl. Assuming you started with 10 molecules of each: a. Draw a picture of what each solution looks like at equilibrium. b. What are the major species in each beaker? c. From your pictures, calculate the Ka values of each acid. d. Order the following from the strongest to the weakest base: H2O, A. Cl. Explain your order.arrow_forward
- What is [OH-] in a solution of 0.125 M CH3NH2 and 0.130 M CH3NH3Cl?. CH3NH2(aq)+H2O(l)CH3NH3+(aq)+OH(aq)Kb=4.4104arrow_forwardWhat concentration of NH4NO3 is required to make [OH]=1.0105 in a 0.200-M solution of NH3?arrow_forwardExplain why a sample of pure water at 40 C is neutral even though [H3O+]=1.7107M . Kw is 2.91014 at 40 C.arrow_forward
- The ion HTe- is an amphiprotic species; it can act as either an acid or a base.. (a) What is Ka for the acid reaction of HTe- with H2O?. (b) What is Kb, for the reaction in which HTe- functions as a base in water?. (c) Demonstrate whether or not the second ionization of H2Te can be neglected in the calculation of [HTe-] in a 0.10 M solution of H2Te.arrow_forwardWhich of the following concentrations would be practically equal in a calculation of the equilibrium concentrations in a 0.134-M solution of H2CO3, a diprotic acid: [H3O+], [OH-], [H2CO3], [HCO3], [CO32-]? N0 calculations are needed to answer this question.arrow_forwardCyanic acid, HOCN, is a weak acid with a Ka value of 3.5 104 at 25C. In a 0.293 M solution of the acid, the degree of ionization is 3.5 102. Calculate the degree of ionization in a 0.293 M solution to which sufficient HCl is added to make it 4.19 102 M HCl in the given volume.arrow_forward
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