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If you add 5.0 mL of 0.50 M NaOH solution to 20.0 mL to Buffer C, what is the change in pH of the buffer? (where buffer C is 8.203 g sodium acetate with 100.0 mL of 1.0 M acetic acid) I have calculated the pH of buffer C to be -
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Determine how many mL of solution A (acetic acid-indicator solution) must be added to solution B (sodium acetate-indicator solution) to obtain a buffer solution that is equimolar in acetate and acetic acid. Solution A: 10.0 mL -
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Pure acetic acid, known as glacial acetic acid, is a liquid with a density of 1.049 g/mL at 25°C. Calculate the molarity of a solution of acetic acid made by dissolving 35.00 mL of glacial acetic acid at 25°C in enough water to -
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Calculate the volume of 1.00 M acetic acid solution and mass of sodium acetate needed to make 250 mL of a 0.450 M acetic acid/acetate buffer solution with a pH of 4.00. (The pKa is 4.74 for acetic acid).
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1.)An ammonia/ammonium buffer solution contains 0.35 M NH3 and 0.72 M NH4+. The Kb value of ammonia is 1.8×10−5. Calculate the pH of this buffer. 2.) Nitrous acid has a Ka of 4.5×10−4. What is the pH of a buffer solution -
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What molar ratio of acetic acid to sodium acetate is required to create a buffer solution having a pH of 4.83 at 25 Celsius? Ka for HC2H3O2 is 1.8 x10^-5 a)0.82 b)0.55 c)3.5 d)1.2 e)2.0 The answer I got was 8.2 ..(help!) -
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What molar ratio of acetic acid to sodium acetate is required to create a buffer solution at a pH of 4.89 at 25 degree C? Ka for acetic acid is 1.8 X 10-5 A. 2.9 B.0.56 C.1.4 D.0.72 E.0.2 ( I chose this and got is wrong) I'm lost -
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A reference calls for the use of "one litre of 0.1 molar acetate buffer pH 5.2” Calculate the amounts of sodium acetate and acetic acid required to make up this buffer, given that for acetic acid Ka = 1.8 x 10-5
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a buffer is made by mixing 0.1 moles of acetic acd a sodium acetate in 500 ml of solution. determine the pH of the buffer. (Ka for acetic acid - 1.8E-5) -
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How would you prepare 30 mL of acetic acid/acetate buffer solution of pH = 5.06?. Assumeyou have 0.1M solutions of both acetic acid and sodium acetate {pKa(acetic acid) = 4.76} -
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You want to make an acetic acid/acetate buffer, pH 3.8, with a volume of 250 mL, and a final concentration of ([AcOH] + [AcO-]) = 0.1 M. You may only use acetic acid and sodium acetate (no strong acid or base). How many mL of -
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What is the pH of a buffer solution if you have 250 ml of a 1.56M Acetic Acid and you added 26.56 grams of sodium acetate (NaCH3CO2)? What is the new pH if you now add 1gram of NaOH to the buffer solution?
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