A 50.0 mL sample of 0.050 M ammonia is titrated with 0.050 M HBr.  Determine the pH of the solution after the addition of 25.0 mL of HBr. KA of ammonium is 5.56 × 10–10 Enter the pH with only 2 sigfigs.

A solution of an unknown weak base (0.495 g in 100 mL of water) was prepared and titrated with standardized 0.113 M HCÌi and the pH of the solution was plotted as a function of titrant added (shown below). Titration of a Weak Base With 0.113 M HCI 12 10 10 20 30 40 50 60 70 80 90 Volume of HCl added (ml) Possible identities for the three liquid bases are shown in the table below. Base pyrole pyrimidine pyridine triethylamine 2.51 x 10-14 1.25 x 10-13 1.70 x 10-9 5.30 x 104 Density (g/mL) 0.967 1.02 0.982 0.762 Based on the data above, identify the weak base and explain your selection. The best explanations will account for all relevant experimental data. Additionally, suggest an indicator to use for this titration if it were to be done without a pH meter. Hd

Consider the titration of 100.0 mL of 0.100 M H2NNH2 (Kb = 3.0 × 10−6 ) by 0.200 M HNO3. Calculate the pH of the resulting solution after the following volumes of HNO3 have been added.a. 0.0 mLb. 20.0 mLc. 25.0 mLd. 40.0 mLe. 50.0 mLf. 100.0 mL

In titrating HC2H3O2 (aq) with 0.1 M NaOH, the equivalence point in pH units will be   A. lower than 7 due to hydrolysis of HC2H3O2  B. lower than 7 due to hydrolysis of Na+  C. higher than 7 due to hydrolysis of C2H3O2-  D. equal to 7 since the acid and base are completely neutralized at the equivalence point.

Calculate the pH of a buffer that is 0.208 M lactic acid, HC3H5O3, and 0.208 M sodium lactate, NaC3H5O3 if 9.474 mL of 4.192 M NaOH is added. The total volume is 1.00 L. The Ka for lactic acid is 1.4*10-4.

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

Determine the pH at the equivalence point of a titration between 50.0 mL of 0.157 M (CH3)2NH solution with 0.157 M HCIO4. Remember that only the decimals in a pH count as significant figures. Please enter your answer with three decimal places.

A 25.0 mL sample of 0.86 M HCOOH is titrated with 0.20 M KOH. What is that pH of the solution at equivalence point ? Ka= 1.77 x 10^-14

You are given a 1.00 L buffer solution that is 0.250 M in HF and 0.250 M in LiF.  Find the pH of the solution after the addition of 0.150 moles of solid LiOH.  Assume no volume change upon the addition of base.  The Ka for HF is 3.5 × 10-4.

A 200.0 mL sample of 0.20 M Sr(OH)2 is titrated with 0.20 M HBr.  Determine the pH of the solution after the addition of 400.0 mL HBr. Enter the pH with only 2 sigfigs.