Consider that benzoic acid is a weak acid which has a Ka of 6.3 x 10-5 . C6H5COOH → C6H5COO- + H+ Calculate the [H+ ] ion concentration of a 0.04 M benzoic acid solution. Use your findings from above, determine the pH of the solution.
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Consider that benzoic acid is a weak acid which has a Ka of 6.3 x 10-5 . C6H5COOH → C6H5COO- + H+ Calculate the [H+ ] ion concentration of a 0.04 M benzoic acid solution. Use your findings from above, determine the pH of the solution.
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- COHSOH(ag) + H2On + CeHsO (aq) + H3O*(a9) Ka= 1.12 x 10-10 (a) Phenol is a weak acid that partially dissociates in water according to the equation above. Write the equilibrium-constant expression for the dissociation of the acid in water. (b) What is the pH of a 0.75 M CaHsOH(ag) solution? (C) For a certain reaction involving CaHsOH(ag) to proceed at a significant rate, the phenol must be primarily in its deprotonated form, C3H5O (eg). In order to ensure that the CsHsOH(aq) is deprotonated, the reaction must be conducted in a buffered solution. On the number scale below, circle each pH for which more than 50 percent of the phenol molecules are in the deprotonated form (CoHsO (aq). Justify your answer. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Justification: (d) CeHsOH(ag) reacts with NaOH(ag). Write a net ionic equation representing this reaction (aka: invasion equation). (e) What is the pH of the resulting solution when 30 mL of 0.40 M CSH5OH(aq) is added to 25 mL of 0.60 M NAOH. Show all work…In the laboratory, a general chemistry student measured the pH of a 0.386 M aqueous solution of nitrous acid to be 1.865. Use the information she obtained to determine the Ka for this acid. Ka(experiment) = In the laboratory, a general chemistry student measured the pH of a 0.431 M aqueous solution of hydrofluoric acid to be 1.741. Use the information she obtained to determine the Ka for this acid. Ka(experiment) =Calculate the pH of each of the following buffered solutions. Ka (HC2H3O2) = 1.8 × 10-5 1. 0.11 M acetic acid/0.26 M sodium acetate pH = 2. 0.26 M acetic acid/0.11 M sodium acetate pH = 3. 0.020 M acetic acid/0.15 M sodium acetate pH = 4. 0.15 M acetic acid/0.020 M sodium acetate pH =
- 9) a) Label each species as an Bronsted-Lowry acid or base. Show the conjugate acid-base pairs. HCO; + H;O* H¿CO; + H2O (aqueous solution) b) Phenol (HC&H50) is a weak acid (Ka= 1.5 x 10*). Write the equilibrium chemical equation, equilibrium constant expression, and calculate the pH of a 0.25 M solution of phenol. 10) Blood is mainly buffered by HCO; /H2CO; (H2CO3, Carbonic Acid, K= 4.4x10 -") buffer system. Calculate the pH of human blood for a carbonic acid concentration of 0.091M and HCO; concentration of 1.00M.Consider the following data on some weak acids and weak bases: acid base Ka K, name formula name formula C;H,N |1.7 × 10~9 4 hydrofluoric acid HF 6.8 × 10 pyridine 10 4.9 x 10 alo 4 hydrocyanic acid НCN ethylamine C2H,NH, | 6.4 × 10 Ar Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the sofution t will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 M C2H5NH3B choose one 0.1 M C5H5NHCI choose one v 0.1 М KI choose one v 0.1 M KF choose onePerform the following to determine the pH of a lactic acid solution. Write the acid/base reaction between lactic acid, HC3H5O3 and water. Write an equilibrium expression for the reaction between lactic acid and water. If the Ka of lactic acid is 3.18 x 10-4, what is the pH of a 0.500 M solution of lactic acid?
- Consider the following data on some weak acids and weak bases: acid base Bo Ka K, name formula name formula acetic acid HCH,CO, 1.8 × 10 -, methylamine CH;NH, 4.4 x 10 -4 HNO, 4.5 x 10 4 ethylamine C,H,NH, 6.4 x 10 * -4 nitrous acid Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have t the solution that will have the next lowest pH, and so on. solution pH 0.1 M CH3NH3CI choose one v 0.1 M NANO2 choose one v 0.1 M KCH3CO2 choose one v 0.1 M C2H5NH3Br choose one v Explanation Check O 2022 McGraw Hill LLC. All Rights Reserved. T 回 0中g W DELL2 Calculate the pH of a 0.355 M solution of propanoic acid, for which the Ka value is 1.30 x 10-5.Consider the following data on some weak acids and weak bases: acid base 9. name formula name formula HNO, 4.5 x 10 C;H;N |1.7× 10 nitrous acid pyridine hypochlorous acid 8. HСIО |3.0х 10 methylamine CH;NH, |4.4 × 10-4 Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 М KCIO v choose one 1 (lowest) 0.1 M C5H5NHCI 3 0.1 M NaNO2 4 (highest) 3 0.1 М KNO3 choose one
- Determine the pH of a 0.774556 M C6H5CO2H M solution if the Ka of C6H5CO2H is 6.5 x 10-5.Consider the following data on some weak acids and weak bases: acid base Bo K. name formula name formula HNO2 |4.5 x 10 -4 -4 nitrous acid ethylamine C2H5NH, 6.4 x 10 hydrofluoric acid HF - 4 6.8 × 10 hydroxylamine HONH, |1.1 × 10 8. Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 М HONHзBr choose one v 0.1 M C2H5NH3CI choose one v 0.1 M NaI choose one v 0.1 M NaF choose one v ?10. Calculate the pH of a solution of CH3NH2(aq) Methylamine, Kb = 4.3x104 that has an initial concentration of 0.20 M? Is it acidic, basic, or neutral solution?