What is the pH of a solution that contains 0.45 M CH3COOH and 0.30 M CH3COONa at 25°C (Ka=1.8 x 10^-5)?
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What is the pH of a solution that contains 0.45 M CH3COOH and 0.30 M CH3COONa...
5. Please calculate the pH of a solution containing 0.40 M CH,COOH and 0.70 M CH3COONa (K, acetic acid = 1.8 X 10"): CH3COOH + H+ + CH3COO CH3COONa → CH3COO + Nat 6. The molar solubility of tin(ll) iodide is 1.28 x 10-2 mol/L. What is Ksp for this compound?
What is the pH of a buffer that consists of 0.45 M CH3COOH and 0.35 M CH3COONa? Ka = 1.8 x 10-5 So the answer is 4.64. However, I was under the impression that it is Ka * (base/acid). So wouldn't that be 1.8 x 10^-5 * (.35/.45)? Isn't the CH3COONa the base? Someone please explain. Thank you.
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Determine the pH of a 0.11 M solution of sodium acetate (CH3COONa) at 25 ° C. (Ka of acetic acid = 1.8 × 10−5.) pH =
A buffer solution is 0.409 M in CH,COOH and 0.249 M in CH3COONa . If K, for CH2COOH is 1.8x10-5, what is the pH of this buffer solution? Submit Answer Retry Entire Group 8 more group attempts remaining NEW Use the References to access important values if needed for this question. A buffer solution is 0.347 M in H3PO4 and 0.233 M in NaH,PO.If Ka for H3PO4 is 7.5 x 10-, what is the pH of this buffer solution? PH...
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1. What is the pH of a buffer consisting of 0.30 M CH3COOH & 0.20 M NACH:COO? Ka= 1.8 x 10-5 2. What is the pH of the buffer with 0.10 M NH3 and 0.20 M NH4NO3? Kl = 1.8 x 10-5 3. What is the pH of a buffer formed from combining 10 mL of 0.250 M HCl with 90 mL of 0.150 M NH3? (K = 1.8 x 10-) 4. Calculate the pH of the solution that results...
Calculate the pH of a 0.051 M solution of sodium acetate(CH3COONa). The Ka for lactic acid is 1.4 x 10-4
What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M CH3COOH with 25.00 mL of 0.050 M CH3COONa? Assume that the volume of the solutions are additive and that Ka = 1.8 x 10-5 for CH3COOH.