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- Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.. How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?Consider the titration of HF (K a=6.7104) with NaOH. What is the pH when a third of the acid has been neutralized?
- Calculate the ratio of [] to [] in blood at a normal pH of 7.40. Assume that this is the only buffer system present. ForAddition of the indicator methyl orange to an unknownsolution leads to a yellow color. The addition of bromthymolblue to the same solution also leads to a yellow color.(a) Is the solution acidic, neutral, or basic? (b) What is therange (in whole numbers) of possible pH values for the solution?(c) Is there another indicator you could use to narrowthe range of possible pH values for the solution?Determine the pH during the titration of 62.0 mL of 0.342 M formic acid (K,- 1.8x104) by 0.342 M KOH at the following points. (Assume the titration is done at 25 °C.) (a) Before the addition of any KOH (b) After the addition of 15.0 mL of KOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 93.0 mL of KOH
- Be sure to answer all parts. Exactly 100 mL of 0.15 M nitrous acid (HNO,) are titrated with a 0.15 M NaOH solution. (a) Calculate the pH for the initial solution. (b) Calculate the pH for the point at which 80.0 mL of the base has been added. (c) Calculate the pH for the equivalence point. (d) Calculate the pH for the point at which 105 mL of the base has been added.Determine the pH during the titration of 67.0 ml of 0.375 M formic acid (K, - 1.8x10 4) by 0.375 M KOH at the following points. (Assume the titration is done at 25 °C.) (a) Before the addition of any KOH (b) After the addition of 17.0 ml of KOH (e) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 101 mL of KOH Submit Show Appresch Show Tutar eA buffer system is prepared by combining 0.406 moles of ammonium chloride (NH4CI) and 0.525 moles of ammonia (NH3). What will the solution pH be if 0.221 moles of the nitric acid (HNO3) is added to the solution. Nitric acid is a strong acid. The K, of ammonia is 1.8 x 10-5. (Two decimal places) Type your answer... I S
- 30.0 mL of titrant is required to reach the equivalence point in the titration with a strong base o f an aqueous sample of formic acid, what is the pH of the titration mixture after (a) 10.0 mL, (b) 15.0 mL, and (c) 20.0 mL of titrant have been added?A 0.345 M of generic weak acid was prepared and has a Kb of 3.91 x 10-10. What is the pH of this weak acid? Use ICE tableCuFrent Attempt in PPogress A buffer is prepared by mixing 48.9 g of NH3 and 48.9 g of NH,Cl in 0.683 L of solution. What is the pH of this buffer, and what will the pH change to if 7.68 g of HCI is then added to the mixture? Your answer is correct. pH of this buffer= 9.62 Hint Your answer is incorrect. The pH change = i (in case of decreasing pH the answer should be negative). Hint MacBook Air
