To plot the deformation curve resulting from 10 mL of 0.1 normal sodium hydroxide with 0.1 normal hydrochloric acid at the following points: a- Before the start of deformation. b- At the midway point of the equivalence point. C at the equivalence point. D - After adding 1 ml of the acid after the equivalence point. The PH values will be as follows * 13, 12.5, 7, 1.2 * 13, 12.5, 7, 2.3 *13.9.2. 7. 2.3

). You are running an experiment and need to keep your solution within a certain pH range:  3.5 +/- 1pH unit.  Choose a buffer system (e.g. a conjugate acid/base) with a pKa in the appropriate range.. Assuming you have 0.2M stock solutions of the acid and conjugate base, calculate the L of each need to make 400 mL of buffer. Describe clearly your protocol for making the buffer solution to the desired pH.   Calculate pH for the following.  Add 100 mL of 0.100 M HCl to pure water Add 100 mL of 0.100 M HCl to the 400 mL of buffer you made Add 100 mL of 0.100 M NaOH to pure water Add 100 mL of 0.100 M NaOH to the 400 mL of buffer you made Please complete the problem

Please complete the calculation of the pH of the equivalence point below. Concentration of NaOH solution = 0.1 mol dm-3. Mean titre (NaOH solution) = 18.95 cm3. Amount of NaOH = 0.00189 moles. Molar ratio of NaOH:aspirin = 1:1. Amount of aspirin = 0.00189 moles. Mass of aspirin (in titration) = 0.341 g. |Mass of aspirin (per tablet) = 0.341 g.

A chemist titrates 80.0 mL of a 0.5108 M benzoic acid (HC H,CO,) solution with 0.3462 M NaOH solution at 25 °C. Calculate the pH at equivalence. pK, of benzoic acid is 4.20. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of NaOH solution added. pH = %3D Continue

50.0 mL of the 0.50 M LIOH is added to 25.0 mL of 0.40 M H2SO4. What is the pH at this point in the titration? H₂SO4 + 2LIOH → Li₂SO4 + 2H₂O pH = [?] Hints: How many moles of H+ and OH- combine? How many moles remain after the reaction? What is the total volume after the reaction? pH at 50 mL base Enter

Determine the resulting pH when 0.003 mol of solid NaOH is added to a 100.0 mL buffer containing 0.13 M HClO and 0.37 M NaClO. The value of Ka for HClO is 2.9 × 10⁻⁸. Determine the moles of the ractant and product after the reaction of the acid and base. (Similar to ICE format but is instead Before (mol), Change (mol), and After (mol) Determine the ICE table for HClO (aq) + H2O - H3O+ + ClO- (aq) Fill in Ka= ? = 2.9 * 10-8 Calculate pH

7. Refer to the following table: Table 2-2. Change in pH of 0.2 M Acetate Buffer after addition of Acid or Base [Base]:[Acid] 0.005:0.195 Addition pH HC1 0.095 mol 3.1 HC1 0.075 0.025:0.175 3.9 HС1 0.05 НС1 0.025 0.05:0.15 4.2 0.075:0.125 4.5 0.1:0.1 0.125:0.075 4.7 NaOH 0.025 mol 4.9 NaOH 0.05 mol 0.15:0.05 5.2 NaOH 0.75 mol 0.175:0.025 5.5 NaOH 0.095 mol 0.195:0.005 6.3 a. Calculate the pH of a 0.2 M acetate buffer (a solution containing 0.1 mol L-' acetic acid and 0.1 mol L-1 sodium acetate), given that the pKa of acetic acid is 4.7. b. What would be the pH value after adding 0.05 mol of NaOH to 1 L of 0.2 mol L1 acetate buffer? c. Compare the pH value in (b) with that obtained after adding 0.05 mol NAOH to 1 L of water (a simple solution of 0.05 mol L-' NaOH). d. How much acid or base can be added to 1 L of the 0.2 M acetate buffer so that the pH does not change appreciably (i.e., what is its buffer range)?

D10)

You are given sodium acetate, NaOH (1 M), NaHCO3, and Na2CO3. Determine which two of these four you will need and then show the calculations of the amount of each to make a buffer of pH 9.9 (hint: using method #3). Assume making 100 ml of a 0.1 M buffer.   Please help! will rate and comment asap!! thank you!..

Calculate the expected pH based on how the solution was prepared, again allowing for any dilution taking place. For Solutions 7 and 8, make sure to take into account the acid–base reaction that occurs when an acid or base is added to the buffer.