8. A 100. mL sample of 0.10 MHCI is mixed with 50. mL of 0.12 M NH.. What is the resulting pH? (K, for NH3 = 1.8 × 10-- 3.07 10.93 1.57 12.43 1.40

A 10.0 ml solution of 0.330 M NH, is titrated with a 0.110 M HCl solution. Calculate the pH after the following additions of the HCI solution: 0.00 ml. 10.0 ml., 30.0 ml., and 40.0 ml.. Round your answer to 3 decimal places. Note: Reference the X, of acids at 25 °C and K, of bases at 25°C tables for additional information. Part 1 of 4 th

1. A 0.36 M hydrocyanic acid (HCN) solution has a pH of 4.87. Give: (a) the balanced equation for the ionization of hydrocyanic acid; (b) K. of HCN; (c) % ionization of HCN. a. b.

The 100. mL of buffer solution is 0.05 M in C2H3O2- and 0.10 M in HC2H302. What is the resulting pH when 20.0 mL of 0.1 M HCl is added to the buffer? Ka of HC2H302 = 1.8x10-5 pH after strong acid added = [?] pH of Soln w/ Acid Enter

When a solution is titrated with an base, an indicator (HIn) changes from yellow to blue (In). The Ka of the indicator is 8.00e - 06. At what pH will the indicator color change first be visible? pH = 6.0969 X 0%

5:48 PM Wed Nov 16 Today 5:48 PM 目。 oint when 15.0 ml. of o. 75% Calculate the pH of a titration at the point when 15.0 mL of 0.15 M NaOH is added to 30.0 mL of 0.20 M HNO3 Edit G ¯¯¯

A buffer solution is prepared that is 0.78 M HCN and 0.14 M NaCN. What is the pH of the solution? (Ka(HCN) = 4.9 × 10−10) 4 sig figs please

Given: 0.300M NaOH            35.0L of 0.450M CH3COOH solution. CH3COOH dissociate constant = 1.8*10^-5 write out the equilibrium equation formed at the equivalence point.

Calculate the pH when 4.0 mL of 2.0 M NaOH is added to the buffer solution containing 25mL of 1.0 M HC,H;O2 and 25mL of 1.0 M NaC2H;O2. Where, K, = 1.8m10-5. 4.75 5.03 4.50 5.25

A 31.1 mL sample of a 0.190 M  solution of NaCN is titrated by 0.230 M  HCl. Kb for is CN- is 2.0x10^-5 Calculate the pH of the solution:   1.  after the addition of 35.7 mL of 0.230 M  HCl