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Calculate the pH and [S2-] in a 0.15 M H2S solution. Assume Ka, 1.0 x 10-7,...
the pH and [s2-1 in a 0.21 M H2S solution. Assume Ka,-1.0x10-7. Ka,-1.0x10-19. Calculate pH [s2-] Calculate the pH of a 3.9x10 M solution of H2SO4 Need Help? Read it the pH and [s2-1 in a 0.21 M H2S solution. Assume Ka,-1.0x10-7. Ka,-1.0x10-19. Calculate pH [s2-] Calculate the pH of a 3.9x10 M solution of H2SO4 Need Help? Read it
Calculate the pH of a 0.982 M solution of hydrogen sulfide (H2S) Where: H2S (aq) -> H+ (aq) + HS- (aq) Ka1 = 1.0 x 10-7 HS- (aq) -> H+ (aq) + S2- (aq) Ka2 = 1.0 x 10-19 Enter your answer with at least 2 sig figs.
Calculate the pH and the equilibrium concentration of S2- in a 7.90×10-2 M hydrosulfuric acid solution, H2S (aq). For H2S, Ka1 = 1.0×10-7 and Ka2 = 1.0×10-19
Calculate the pH after 0.16 mole of NaOH is added to 1.06 L of a solution that is 0.46 M HNO2 and 1.14 M KNO2, and calculate the pH after 0.32 mole of HCl is added to 1.06 L of the same solution of HNO2 and KNO2. 0.16 mole of NaOH 0.32 mole of HCl 12. 6.25 points | Previous Answers ZumChemP8 8E.029 My Notes Ask Your Calculate the pHfter 0.16 mole of NaOHs added to 1.06 L of a...
determine the pH of a solution that is 0.15 M HClO2 (Ka=1.1 x 10^-2) and 0.15 M HClO (Ka=2.9 x 10^-8).
The ionization constants for the diprotic acid H 2S are 1.0 x 10 -7 and 1.3 x 10 -13. H2S (aq) + H2O (l) <=> HS -(aq) + H3O +(aq) Ka = 1.0 x 10 -7 HS -(aq) + H2O (l) <=> S-2 (aq) + H3O +(aq) Ka = 1.3 x 10 -13 What is the equilibrium concentration of HS - in a 0.300 M solution of H2S?
Given that Ka for HCN is 6.2*10^-10, calculate the pH of a 0.15 M KCN solution.
Calculate the pH of a 0.15 M CH3COOK solution. (Ka for acetic acid = 1.8 × 10−5.)
Calculate the pH of a 0.10 M NaHX salt solution. Ka (H2X) = 7 x 10-5 Ka (HX-) = 5.3 x 10-11
2. Calculate the pH of a 0.230 M calcium acetate solution if the Ka for acetic acid is 1.8x10-5 . 3. Calculate the pH of a 0.225 M solution of H2CO3. Ka1 = 4.3x10^-7 ; Ka2 = 5.6x10^-11 4. Calculate the pH of a 0.0080 M solution of sulfuric acid. Ka2 = 1.2x10^-2