Concept explainers
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Concept Introduction:
(b)
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(c)
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(d)
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(e)
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Concept Introduction:
The negative log of base 10
Equilibrium constant for base dissociation in aqueous solution is,
The general base dissociation reaction in water is,
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General Chemistry: Atoms First
- Consider the titration of a 50.00 mL sample of 0.500 M hydrazoic acid, HN3, with 0.500 M NaOH (aq., 25 oC). The Ka HN3 = 4.50 x 10–4. What is the pH of the solution after 15.00 mL of NaOH has been added?arrow_forwardAt 22 °C, an excess amount of a generic metal hydroxide, M(OH)2, is mixed with pure water. The resulting equilibrium solution has a pH of 10.16. What is the Ksp of the salt at 22 °C?arrow_forwardConsider the titration of a 50.00 mL sample of 0.100 M ethylamine, C2H5NH2, with 0.100 M HCl (aq., 25 oC). The Kb C2H5NH2 = 6.41 x 10–4. What is the pH after 25.00 mL of HCl has been added?arrow_forward
- Calculate the molar solubility (aq., 20 oC) of aluminum hydroxide, Al(OH)3, in 0.000852 M NaOH. The Ksp of Al(OH)3is 2.0 x 10–32.arrow_forwardThe half-equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.480 moles of a monoprotic weak acid (Ka = 5.3 x 10-5) is titrated with NaOH, what is the pH of the solution at the half-equivalence point?arrow_forwardSketch reasonably accurately the pH curve for the titration of 25.0 cm3 of 0.15 M Ba(OH)2(aq) with 0.22 M HCI(aq). Mark on the curve (a) the initial pH, (b) the pH at the stoichiometric point.arrow_forward
- A 20.00 mL aliquot of lactic acid solution (HCH3H5O3) was titrated with 0.0980 M KOH(aq) using both an indicator and a pH meter. Ka (HCH3H5O3), is 1.38 x10-4. A total of 28.64 mL of 0.0980 M KOH(aq) was required to reach the equivalence point 1. Calculate the molarity of the lactic acid solution. 2. Calculate the pH of the lactic acid solution 3. Calculate the pH and [CH3H5O3-] at the half-equivalence point. 4. Calculate the pH at the equivalence point of the titration. 5. Suggest an appropriate indicator for titration. 6. Calculate the pH of the solution after 10.00 mL of 0.0980 M NaOH(aq) was addedarrow_forwardBenzoic acid, C6H5COOH, dissociates in water as shown in the equation below. A 40.0 mL sample of an aqueous solution of benzoic acid with a concentration of 0.50 M is titrated using standardized 0.25 M NaOH. C6H5COOH(s) -> C6H5COO–(aq) + H+(aq) Ka = 6.46 x 10^-5 Calculate the pH of the solution after the following amounts of NaOH have been added… A. 0 mL B. 10 mL C. 85 mLarrow_forwardThe half-equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other hall still remains unreacted if 0.360 moles of a monoprotic weak acid (K, = 4.8 x 10^-5 ) is titrated with NaOH, what is the pH of the solution at the half -equivalence point? pH =arrow_forward
- A student does a titration of 86.0 mL of a 0.37 M solution of methylamine (CH3NH2(aq) (pKb =3.36) with HCl(aq). When 100 mL of HCl had been added to the mixture, the pH was measured and found to be 9.54. What was the molarity of the HCl solution?arrow_forwarda.) A student titrated 50.0mL of a 0.10M solution of a certain weak acid with NaOH(aq). The results are given in the graph attached. (i) What is the approximate pKa of the acid? (ii) What specific value from the graph is needed, in addition to the information in part (a) above, to calculate the molar concentration of the NaOH(aq) ? (iii) Identify a pH value between 2.5 and 7.5 at which the concentration of the weak acid being titrated is less than the concentration of its conjugate base.arrow_forwardFor a titration to be effective, the reaction must be rapid and the yield of the reaction must essentially be 100%. Is Kc > 1, < 1, or ≈ 1 for a titration reaction?arrow_forward
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