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

In which on e of the following solutions is silver chloride the most soluble? A) 0.0150 M NH3 B) 0.200 M HCl C) pure water D) 0.750 M LiNO3 E) 0.185 M KCl

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 standard deviation for the answer of the following mathematical operation. The number between brackets is the standard deviation of the preceding number. 90.0 ( 2.0)/40.0 (2 4.0) 2.25 ( ??)