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Chemistry
Acid-Base Equilibrium
pH Calculation
calculate the pH when 10 mL of .511 M sodium acetate and 20.00 mL of 0.350 M acetic acid
1 answer
Use the Henderson-Hasselbalch equation.
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calculate the molarity of sodium in 12.4g of sodium acetate diluted in 100mL of ID water, and calculate concentration of both
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I will be happy to critique your thinking.
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Calculate the amounts and pH values for preparing the following acetic acid/acetate buffer solution.
1.) In the first step, If
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I think something is missing here. I don't get the connection between step 1 and step 2 and the
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calculate the molarity of sodium in 12.4g of sodium acetate diluted in 100mL of ID water? and calculate concentration of both
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duplicate.
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You are preparing 500 mL of a 0.300 M acetate buffer at pH 4.60 using only sodium acetate, 3.00 M HCl, 3.00 M NaOH, and water.
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pH = pKa + log(base)/(acid) 4.60 = 4.74+ log b/a b/a = about 0.7 but that's approximate and you need
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Calculate pH of an acetate buffer containing 27.5 mM acetic acid (pKa is 4.74) and 50 mM
sodium acetate. When a 30 mM aq solution
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I worked this below. I can find it if you wish.
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1. Calculate pH of an acetate buffer containing 27.5 mM acetic acid (pKa is 4.74) and 50 mM sodium acetate. When a 30 mM aq
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a. pH = 4.74 + log(base)/(acid) = approx 5.00 b. millimoles NaAc = mL x M = 500 mL x 0.030M = = 15
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anyone know how to do this and which choice is correct?thank you so much in advance.
Use the Henderson-Hasselbalch equation to
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Use the Henderson-Hasselbalch equation. ou will need pKa for acetic acid. The base in the HH
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a flask containing 50ml of 0.128M sodium acetate is titrated with 0.138M nitric acid. Calculate the initial ph of the acetate
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a. I will call acetate Ac^-. ......Ac^- + HOH ==> HAc ==> OH^- I...0.128.............0......0
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given 6.7 grams of sodium acetate and 6.7 g of magnesium acetate, calculate the number of moles of acetate in sodium acetate.
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moles = grams/molar mass moles Ac in NaAc = grams/molar mass. In Mg(Ac)2, it is moles Mg(Ac)2 =
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