Determine the pH of an aqueous solution at 25 ° C that was formed with 0.06 mol / L of KCN and 0.02 mol / L of CH3COOH. Using CH3COOH Ki = 1.8x10-5 , and HCN Ki = 4x10-10

||| ctrl lacc shift ↑ tab caps lock VILION Mc ALE Graw HI esc K →1 Pavilion x360 fn O CHEMICAL REACTIONS Determining the molar mass of an acid by titration McCA X Eplanation g mol V An analytical chemist weighs out 0.188 g of an unknown triprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1500M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 38.4 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. f1 Type here to search A https://www-awu.aleks.com/alekscgi/x/Isl.exe/1o_u-IgNslkr7j8P3jH-IvUrTNdLZh5A8CnG03PBGuXr8iCPa7ZMmym f2 @ Z Check 2 L M W hp S ALE MCCA ALER f3 # Mc Graw 3 X alt D 4 $ 4 с x10 X R O f5 Me Graw MI % F 5 at 40 MCCA ALE ALE ● V T S f6 4- G 6 ■ T f7 B Y ♫+ & Mc 7 H raw fg MCCA ALER *. N KAA © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center |…

Ka of acetic acid equals 1.8*10^-5 The buffer solution is 50 mL of 0.2 M CH3CO2H and 50 mL of 0.2 M NaCH3CO2together in a beaker.  What is the theoretical pH of each soluton? a. 50 mL of boiled deionized water + 5 mL of 0.2 M HClb. 50 mL of boiled deionized water + 5 mL of 0.2 M NaOHc. 50 mL of buffer + 5 mL of 0.2 M HCld. 50 mL of buffer + 5 mL of 0.2 M NaOH

The temperature for each solution is carried out at approximately 297 K where Kw=1.00 x 10-14-   a) 0.20 g of hydrogen chloride (HCl) is dissolved in water to make 4.5 L of solution. What is the pH of the resulting hydrochloric acid solution? Express the pH numerically to two decimal places.   b)  0.70 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 3.0 L of solution. What is the pH of this solution?   Express the pH numerically to two decimal places.