You have a 825.3 mL sample of 2.754 M HA (Ka = 4.49⋅10−4). Calculate the pH of the best buffer.
You have a 825.3 mL sample of 2.754 M HA (Ka = 4.49⋅10−4). Calculate the pH...
Calculate the pH of a buffer solution when 65.0 mL of 0.215 M weak acid (HA) is mixed with 25.0 mL of 0.215 M NaOH. The Ka for HA is 6.3x10-5.
So equation 15 is [H+]= Ka• [HA]/[A-] Basically, we desire to have a ph of 4.7, from an acid of 0.1M and a conjugate base of 0.1M. Ultimately our solution should have a total volume of 0.01 L, and we have a ka of 3.04x 10^-5. However I do not know how to find [HA]/ [A-] in the the buffer and how to find the volume of 0.1 M HA/ volume 0.1 M A- needed on buffer. Neither volumes are...
1. Determine the pH of a buffer solution prepared by mixing 25.3mL of 0.35M HA (Ka= 1.6x10-5) with 15.3mL of 0.45M NaA. 2.100 mL of buffer solution that is 0.15M HA (Ka= 6.8x10-5) and 0.20M NaA is mixed with 17.3mL of 0.25M HCl. What is the pH of the resulting solution? 3. Calculate the pH of a solution made by mixing 75.0mL of 0.15M HA (Ka= 2.5x10-5) with 7.5mL of 0.75M NaOH 4. 100 mL of buffer solution that is...
1) You have 50 mL of a buffer solution that is 0.15 M in HA and 0.25 M in A-. Calculate the pH of the solution after you add 100 mL of 0.01 M HCl to the solution. The pKa of HA is 4.75. 2)You wish to prepare 100 mL of a buffer solution that is 0.025 M in carbonic acid (H2CO3). The pKa of H2CO3 is 6.351. Calculate the amount of H2CO3, in grams, that you will need to...
Calculate the pH when 59.0 mL of 0.271 M of a certain monoprotic weak acid, HA, is mixed with 59.0 mL of 0.271 M sodium hydroxide solution at 25 °C. For HA, the Ka is 8.5× 10–5 M
Calculate the pH when 65.0 mL of 0.269 M or a certain monoprotic weak acid, HA, is mixed with 65.0 mL of 0.269 M sodium hydroxide solution at 25 degree C. For HA, the Ka is 1 .5x 10^-5.
Find the volume of HA/Na is needed for the buffer when we have a desired ph of 4.7, a ka of 3.04• 10^-5, and a total volume of 10 ml. We do not know the volume of HA or NA, that is what we are trying to find ements Target pH of buffer solution to be prepared 4.7 ph Average value of K (average of the three K values above) K = 3.04x16 5 [HA] A-T in buffer 200...
37. You have 500.0 mL of a buffer solution that is 0.30 M HF and 0.50 M KF. Ka for HF is 7.1 x 10-4 a) Calculate the pH of the buffer. b) Calculate the pH of the buffer after adding 0.020 moles of HCI. c) Calculate the pH of the buffer after adding 0.030 moles KOH. - -Loel.
A 40.0 mL sample of 0.150 M HNO2 (Ka = 4.60 x 10-4) is titrated with 0.200 M KOH. Calculate: a. the pH after adding 10.00 mL of KOH b. the pH at one-half the equivalence point c. the pH after adding 20.00 mL of KOH d. the volume required to reach the equivalence point e. the pH at the equivalence point f. the pH after adding 45.00 mL of KOH
You have 75.0 mL of 0.150 M HNO2 (Ka = 4.50 x 10-4) to which you add 50.0 mL of 0.150 M NaOH. What will be the resulting pH of the solution?