A solution of 0.25 M potassium hydroxide, KOH is added from a burette to a flask containing 25.0 mL of 0.20 M weak acid, HA. The titration curve is divided into regions I and II as shown below. PH 11 Volume of titrant Choose the incorrect statement about this titration. O The buffer region is labelled I and II. O O O The volume of KOH at the equivalence point is 20.0 mL. The pH at the equivalence point is larger than 7. The species present at region I are HA and A.

2. A beaker with 100.0 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 7.30 ml of a 0.360 M HCI solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.752.

You have 100 mL of an acetic acid/acetate buffer. The solution is comprised of 0.33 M acetic acid and 0.01 M acetate. What is the new pH when 5.0 mL of 0.10 M HCl is added to this solution? The pKa of this pair is 4.76. (Note: You must use the I.C.E method for this one).

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.

A 50.0 ml. sample of 0.15 M NH, is titrated with 0.10M HCI, Determine the equivalence point of this titration. The K of NH3 is 1.8 x 10 O 75.0 ml O 87.6 ml O 90.3 ml O 50.0 ml O 39.5 ml.

Suppose there is 1.00 L of an aqueous buffer containing 60.0 mmol of acetic acid (p?a=4.76) and 40.0 mmol of acetate. Calculate the pH of this buffer. pH=     What volume of 2.50 M NaOH would be required to increase the pH to 4.93? volume:

Calculate the pH of a buffer that initially contains 6.50×10-4 M HOCl and 7.50×10-4M NaOCl. The Ka of HOCl is 3.0×10-5

A beaker with 195 mLmL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 MM.  A student adds 7.70 mLmL of a 0.440 MM HClHCl solution to the beaker. How much will the pH change? The pKapKa of acetic acid is 4.740. Express your answer numerically to two decimal places. Use a minus ( −− ) sign if the pH has decreased.

Please don't provide handwriting solution

c) If 30 ml of 0.15 M HOCE is titrated with 0.20 M NaOH, I) Write a balanced equation for the reaction and calculate the volume of NaOH required to reach the equivalence point. I) Sketch the titration curve for the above reaction. Label the axds, the buffer region and the approximate equivalence point. I) From the list below, select the most sultable indicator for the titration. Methyl red: Cresol red: Thymol-phthalein: pH 4.2 (red) - pH 8.3 (yellow) pH 6.8 (yellow) - pH 8.5 (red) pH 9.4 (colourieses) – pH 10.6 (blue)