Science Chemistry
If the Ka of a monoprotic weak acid is 9.0 × 10-6, what is the pH of a 0.26 M solution of this acid?
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Weak Acid 1.) The pH of a 0.060M weak monoprotic acid HA is 3.44. Calculate the Ka of the acid. 2.) The pH of 0.100M solution of
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Weak Acid 1.) The pH of a 0.060M weak monoprotic acid HA is 3.44. Calculate the Ka of the acid. 2.) The pH of 0.100M solution of
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I have shown you how to do these below. If you want to post your answer I can check it
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the initial acid molarity is ... [HA] = .112 * (22.32 / 25.00) = 0.100 [H+] = 10^(-2.87) = .00135
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So (H^+) = 0.04 x 0.14 = ?? (X^-) is the same. (HX) = either, 0.04-(0.04*0.14) OR 0.04*0.86 (HX)
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A. Strong Base 1.) What is the concentration of a solution of KOH for which the pH is 11.89? 2.) What is the pH of a 0.011M
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a) HA + NaOH ==> H2O + NaA b) moles NaOH = M x L = ?? Using the coefficients in the balanced
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NaOH + HA ==> NaA + H2O mols NaOH = M x L = ? mols HA = mols NaOH (look at the coefficients) M HA =
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......HA ==> H^+ + A^- I.....0.5....0......0 C.....-x.....x......x E...0.5-x....x......x Enter the E
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To determine the molar concentration of the weak acid solution, we need to use the concept of
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