calculate the number of grams of CH3COONa * 3H2O (sodium acetate tri-hydrate) needed to make 250.0 mL of a CH3COOH (acetic acid)/ CH3COONa * 3H2O buffer. The target pH of the buffer is 5.25. The given concentration of [CH3COOH] is equal to 0.10 M. Ka = 1.80 x 10-5 for acetic acid. PLEASE EXPLAIN :(
Q1:Given the Ka value in the instructions (1.80 x 10-5). Calculate the pKa
Q2:Use the Henderson-Hasselbalch equation to determine the ratio of [CH3COO-]/[CH3COOH] needed to make the buffer. pH = pKa + log([CH3COO-]/[CH3COOH])
Q3:Now calculate the concentration of acetate ion (CH3COO- ) needed to make the buffer. Hint: Recall the concentration of CH3COOH given in the instructions.
Q4:Now, give the concentration of CH3COONa * 3H2O needed to make the buffer. Hint: The CH3COONa * 3H2O dissolves in water to form Na+ ions and CH3COO-.
Q5:Finally, convert the concentration of CH3COONa * 3H2O into grams of CH3COONa * 3H2O needed to make the buffer.
Acidic buffers are solutions that have a pH below 7 and contain a weak acid and one of its salts. For example, a mixture of acetic acid and sodium acetate acts as a buffer solution
calculate the number of grams of CH3COONa * 3H2O (sodium acetate tri-hydrate) needed to make 250.0...
calculate the number of grams of CH3COONa * 3H2O (sodium acetate tri-hydrate) needed to make 250.0 mL of a CH3COOH (acetic acid)/ CH3COONa * 3H2O buffer. The target pH of the buffer is 5.25. The given concentration of [CH3COOH] is equal to 0.10 M. Ka = 1.80 x 10-5 for acetic acid. Use the Henderson-Hasselbalch equation to determine the ratio of [CH3COO-]/[CH3COOH] needed to make the buffer. pH = pKa + log([CH3COO-]/[CH3COOH]) Now calculate the concentration of acetate ion (CH3COO-...
How many grams of sodium acetate, CH3COONa, is required to mix with 2.00 Liters of 0.450 M acetic acid, CH3COOH, in order to prepare a buffer solution with a pH that equals 5.00? pKa(CH3COOH) = 4.74 and molar mass(CH3COONa) = 82.03 g/mol
Calculate the grams of sodium acetate required to make 250.0 mL of a pH 5.50 buffer solution using 0.100 M acetic acid (Ka of 1.8x10-5).
Calculate the volumes of 0.20 M acetic acid and 0.20 M sodium acetate needed to make 20.00 mL of a buffer having pH = 5.00. Repeat analogous, separate calculations for buffers having pH = 4.00 and pH = 6.00. Hint: set up two equations with two unknowns; the first is the Henderson-Hasselbalch equation, the second is the fact that the volumes of HA (x mL) and A− (y mL) solutions should sum to 20 mL. In the Henderson-Hasselbalch equation, use...
7. Calculate the mass of sodium acetate (CH3COONa) that must be added to 1.00 L 0.450 M acetic acid (CH3COOH), Ka = 1.8 x 10 ) to form a pH = 5.00 buffer. Ka = 1.8 x 109.
what concentration of acetic acid (pka=4.76) and acetate would be required to prepare a .15 M buffer solution at pH 5.0? What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.15 M buffer solution at pH 5.07 Note that the concentration, the pH, or both values may differ from that in the first question. Strategy 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid). (AVHA)....
Calculate the amounts in grams of weak acid and conjugate base needed to make the buffer. Buffers Concentration Volume Weak Acid Conjugate Base sodium acetate pH Ka acetic acid Buffer 1 500 mL 4.75
Acetic acid (CH3COOH,CH3COOH, ?a=5.62×10−5)Ka=5.62×10−5) is a weak acid, so the salt sodium acetate (CH3COONa)CH3COONa) acts as a weak base. Calculate the pH of a 0.445 M0.445 M solution of sodium acetate.
Resources Ex Give Up? What concentrations of acetic acid (pka = 4.76) and acetate would be required to prepare a 0.15 M buffer solution at pH 4.92 Note that the concentration, the pH, or both values may differ from that in the first question. Strategy 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid), [ A HA). 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate...
What concentrations of acetic acid (pKa 4.76) and acetate would be required to prepare a 0.10 M buffer solution at pH 4.5? Note that the concentration and/or pH value may differ from that in the first question. STRATEGY 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration of acetic acid Step 1: Rearrange the Henderson Hasselbalch...