A solution of a weak acid is titrated with a standard solution of a strong base. The progress of the titration is followed with a pH meter. Which of the following observations best describes what would occur? Initially the pH of the solution increases slowly, and then it increases much more rapidly, before increasing slowly again At the equivalence point, the pH is 7 The pH of the solution gradually decreases throughout the experiment After the equivalence point, the pH becomes constanc because this is the buffer

1. A buffer solution contains 0.419 M of ammonium chloride and 0.221 M of ammonia.If 0.0293 moles of sodium hydroxide are added to 150 mL of this buffer, what is the pH of the resulting solution? (Assume that the volume does not change upon adding sodium hydroxide.) 2. A buffer solution contains 0.286 M of ammonium chloride and 0.472 M of ammonia. If 0.0620 moles of nitric acid are added to 250 mL of this buffer, what is the pH of the resulting solution? (Assume that the volume does not change upon adding nitric acid.)

Equimolar quantities of lithium hypochlorite and hypochlorous acid are placed into solution. What happens to the buffer system if some sodium hydroxide is added to the solution? ) The sodium hydroxide reacts with the hypochlorite ion and the pH decreases significantly. The sodium hydroxide reacts with the hypochlorious acid and the pH increases significantly. The sodium hydroxide reacts with the hypochlorite ion and the pH decreases only slightly. The sodium hydroxide reacts with the hypochlorious acid and the pH increases only slightly.

What is the general composition of a buffer and in your own words explain why it resists change in PH.

A student is titrating a 100 mL of 0.50 M solution of hydrofluoric acid (HF) with 1.0 M strong base (NaOH). a) at the equivalence point, what ions/compounds will be present in the solution? A complete answer will also be specific as to what ions/compounds are not present in solution. b) calculate the pH at the equivalence point.

Consider a solution of a weak acid  being titrated with a solution of a strong base to beyond the equivalence point. Which of the following statements is incorrect?   a. The pH will increase intially and then change very little until the equivalence point is reached   b. Only a small percentage of the weak acid will react with the added base   c. The volume of the base solution required to reach the equivalence point can be less than, equal to, or more than the volume of the acid solution.   d. At the equivalence point, the solution will be basic   e. Beyond the equivalence point, the solution will be basic   f. None of the above   g. The pH of the solution in the tiration flask is affected by the total volume at any given point

In this lab, we will experimentally determine the titration curve for the titration of a weak acid solution against a strong base solution. The weak acid we will use is potassium hydrogen phthalate, KHP, its chemical structure is shown below. KHP is an ionic compound composed of a potassium cation K+ and a hydrogen phthalate anion HP–. HP– is a weak acid and upon dissolving in water, can lower the pH of the solution. (a)  Suggest the chemical reaction(s) when a solid sample of KHP is dissolved in water, writing out the chemical equations for them. (b)  Sketch the structure of KHP from above and circle the hydrogen atom that is responsible for its acidity. (c)  Calculate the pH of a solution made of 0.50 g of KHP and 50 mL of water. KHP has a molar mass of 204.2 g and at 25 °C has a pKa of 5.4.

theoretically, the equivalence point and end point of a titration should be the same. Describe four factors that could be responsible for the difference between these two in an actual titration

Determine the pH during the titration of 21.9 mL of 0.277 M perchloric acid by 0.206 M sodium hydroxide at the following points: (1) Before the addition of any sodium hydroxide (2) After the addition of 14.8 mL of sodium hydroxide (3) At the equivalence point (4) After adding 35.4 mL of sodium hydroxide

(Answer highlighted questions please) A 50.050.0 mL solution of 0.1390.139 M KOHKOH is titrated with 0.2780.278 M HClHCl. Calculate the pH of the solution after the addition of each of the given amounts of HClHCl. 20.0 mLpH=20.0 mLpH=     24.0 mLpH=24.0 mLpH=     25.0 mLpH=25.0 mLpH=