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complete and balance each of the following equations for acid base reactions
HClO4 (aq) + NaOH (aq) ------>
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- For part, b would the calculations be the same for NO3^- (aq) and CO^2+ (aq), meaning those species PH would also equal 0?Calculate the pH of a solution prepared by dissolving 1.15g of sodium acetate, CH3COONa, in 95.5 mL of 0.10 M acetic acid, CH3 COOH(aq). Assume the volume change upon dissolving the sodium is negligible. Ka of CH3COOH is 1.75 x 10-5.Estimate the pH of 1.5 x 10-4 M CH3COOH (aq), being careful to treat this solution as dilute, and not open to the approximations used as given below.
- Calculate the pH of a solution prepared by dissolving 1.75 g of sodium acetate, CH3COON,, in 53.5 mL of 0.15 M acetic acid, CH3COOH(aq). Assume the volume change upon dissolving the sodium acetate is negligible. Ka of CH3COOH is 1.75 x 10-5.500 mL of 0.291 M NaOH(aq) are mixed with 500 mL of 2.00 M HCOOH(aq). What is the pH of the resulting solution, if the acid ionization constant for formic acid is 1.7*10-4?The Ka value for acetic acid, CH3COOH(aq), is 1.8×10−5. Calculate the pH of a 2.80 M acetic acid solution
- The pH of an aqueous solution of acetic acid (CH3COOH) is 2.0. What is the initial molar concentration of CH3COOH, if its acid ionization constant is Ka = 1.8×10–5?Calculate the pH of the following acid solutions at 25 °C: (a) 1.0 x 10-4 M H3BO3(aq) (boric acid acts as a monoprotic acid), (b) 0.015 M H3PO4 (aq), (c) 0.10 M H2SO3(aq). Values for the successive acidity constants for each of these acids are given in the below table.calculate the pH of a solution prepared by dissolving 1.45g of sodium acetate, CH3COONa, in 99.0mL of 0.10M acetic acid, CH3COOH(aq). Assume the volume change upon dissolving the sodium acetate is negligible. Ka of CH3COOH is 1.75x10^-5