last

Consider a strong acid-weak base titration between 0.250 M HNO3 and NH3. a. The volume of HNO3 added at the equivalence point is 20.50 mL. Calculate the number of moles of HNO3 used in the titration. 5.125e-3 b. Calculate the number of moles of NH3 in the flask 5.125e-3 c. Find the concentration of NH3 in the solution, if 25.00 mL of NH3 is used in the titration. 0.205 mol L-1 d. What is the species present at the equivalence point? e. Find the concentration of the salt present at the equivalence point. f. The Kh of NH3 is 1.8 x 10-5. What is the Ka of NH4*?| g. Find the concentration of H* at the equivalence point. h. Calculate the pH and pOH of the solution at equivalence point pH = pOH = |

Calculate the pH of a titration of 50.00 mL of 0.100 M Phenylacetic acid, Ka = 4.9 x 10-5, with 0.100 M NaOH at the following points: a. Before any NaOH is added.      b. After 18.7 mL of NaOH are added.   c. After 25.00 mL of NaOH are added.   d. After 50.00 mL of NaOH are added.   e. After 53.00 mL of NaOH are added.   C) What is the pKa of the acid (show calculation)? please solve sub-parts a,b, and c.

Suppose that 50.00 mL of 0.100 M acetic acid is titrated with 0.100 M NaOH. (Weak Acid - Strong Base Titration) Find the pH if the following volume of NaOH are added. i. 30 mL NaOH ii. 35 mL NaOH iii. 40 mL NaOH iv. 45 mL NaOH v. 50 mL NaOH

Let HA represent a weak acid. A 27.5 mL sample of 0.20 M HA was titrated with 0.25 M NaOH. The following data were collected during the titration. Volume NaOH added (mL) 5.50 11.00 16.50 22.00 pH 5.28 5.88 6.48 9.98 What is the K, for HA? 5.2 x 10-6 None of these 1.0 x 10-10 3.3 x 10-7 1.3 x 10-6

1. A solution of a weak acid was tested with the indicators used in this experiment. The colors observed were as follows: Methyl violet violet Thymol blue Methyl yellow What is the approximate pH of the solution? orange red 3. The pH of a 0.10 M HOBr solution is 4.8. a. What is [H+] in that solution? Congo red Bromcresol green 2. An aqueous solution of NH, has a pH of 11.6. The ammonia (NH,) molecule is the conjugate base of the NH₂* (called "ammonium") ion. Write the net ionic equation for the reaction that makes an aqueous solution of NH, basic. (Eq. 5.) b. What is [OBr ]? V hat is [HOBr]? (Where do the H+ and OB violet yellow C. What is the value of K, for HOBr? What is the value of pK,? ions come from?) M; M M

Please calculate the pH of a buffer solution made up of formic acid and sodium formate. The solution was made by dissolving 0.808 mol of sodium formate, and 0.808 mol of formic acid in 1.80 Liter of water (please assume a total volume for the solution of 1.80 L). (Ka = 1.80 x 10-4) a. pH= 1.93 Ob. pH = 2.11 Oc. pH = 3.08 d. pH = 3.74 QUESTION 2 The Ka for Formic Acid = 1.80 x 10-4. What is the pH of a 0.778 M Formic Acid solution? HA +B+ A + HB+ Oa. pH = 2.11 b. pH = 1.57 c. pH = 1.93 d. pH = 1.81

a 20.70mL sample of 0.64 M HCL is titeares with 0.64M NaOH. Calculate the pH after the addition of 19.38 mL NaOH

Suppose you titrate NH3 with HC1. With 25.00 mL of NH3 in the flask, it takes 25.00 mL of 0.100 M HCl to reach the equivalence point. Calculate the molarity of ammonia. a. At this equivalence point, what is the pH? (Hint: the Ka for NH4* is 5.6×10-10).

A 600.0 mL sample of 0.20 M HF mL of NaOH. The Ka of HF is 3.5 × 10-4. titrated with 0.10 M NaOH. Determine the pH of the solution after the addition of 600.0 4.15 4.33 3.15 3.46 2.08