pH = 4.7
Ka = 3.04 x 10^-5
pKa = -log Ka = 4.517
concentration of HA = NaA = 0.10 M
volume of HA = x
volume of NaA = 10 - x
pH = pKa + log [salt / acid]
4.7 = 4.517 + log [10 - x / x ]
[10 - x / x ] = 1.524
10 - x = 1.524 x
x = 3.96
volume of HA = 3.96 mL
volume of NaA = 6.04 mL
Find the volume of HA/Na is needed for the buffer when we have a desired ph...
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...
how to find the volume 0.01MHA used and 0.01M NaA used in
ml?
Target pH of buffer solution to be prepared 9.24 K = 3.65 x 100 Average value of K (average of the three K, values above) (HA) in buffer R 1.018 [A-] Hint: use Equation (15) Volume 0.10 M HA 1.018 Volume 0.10 M NA needed in buffer Volume 0.10 M HA used 95 mL Volume 0.10 M NaA used ml Measured pH of prepared buffer 9.57 (4.9x10-10)...
PART C. Properties of Buffers Buffer system selected_HCO -(0,2- Weak acid name _ NaC,H,O, pH of buffer 4.68 (H') = 2.09 XIOK 2.09x10 pH of diluted buffer 4.13 [H") = 1.8x10K - 1.8x10-5 pH after addition of five drops of NaOH 4.76 pH after addition of five drops of HCI - 4.69 pH of buffer in which (HA) = 0.10 5.66 K.- 2.188x106 pH after addition of excess NaOH 11.53 (2.188x10-6) (0.00) pH of distilled water 8.22 10.09) pH after...
You are asked to prepare 10.00 mL of a buffer solution consisting of 0.10 M weak acid (HA) and 0.10 M conjugate base (A-). The target pH of the buffer solution is 5.25. The Ka of HA is 5.0x10^-6. What volume of HA is required to make the buffer?
A buffer solution of pH 5 is needed for an experiment which can be prepared by mixing a weak acid and a strong base. Calculate the volume of a 0.56 M NaOH solution that needs to be added to 50.00 mL of a 0.18 M acetic acid (CH3COOH) solution to obtain a buffer solution of pH 5.00. Ka (CH3COOH) = 1.75 x lO'5]
appropriate sig figs!!! please
Youve been asked by your research advisor to prepare 250.00 mL of a 0.020 M buffer. The target pH is 5.60. The components are C3Hs02 HC3Hs02 and the Ka of the weak acid is 1.3 x 105. Part A what volume (in mL) of a 0.050 M C3H502-solution is taquired to prepare the desired buffer? ml Submit Request Answer Part B What volume (in mL) of a 0.050 M HC Hs02 solution is required to prepare...
Determine the volume you would need of each solution (acid/base and conjugate) to make a buffer with a specific pH. Please only use the acids, bases and salts from the table on page 87 in the lab manual. See below for assigned values, each person will be calculating volumes needed for an acidic buffer and a basic buffer. Chart from page 87 List 0.10 M CH,NH, 9.75 the 0.10 M NHỰC H. " List E 0.10 M HCOOH K -...
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.
pH
of 9.2
using ammonium nitrate: pKa= 9.24
2 Introduiction The Henderson-Hasselbalch equation, or A-1 HAl relates the pH of a buffer with the pKo of the acid and the concentration of the conjugate base A- and the monoprotic acid HA. In cq. (1), pH-_ log[H+], pK, =-log Ka, and [J]i and [JIe are the initial and equilibrium molar concentration of the Jth species, respectively. The buffering capacity of the buffer is given by [1] Ka H+ where K,e-1.0 ×...
Calculate the volume of 3 M HCl needed to change the pH of 75 mL of the undiluted buffer solution by one pH unit (buffer capacity). The undiluted solution was prepared using 100 mL of 1.0870M acetic acid and 100mL of 1.0027M sodium acetate.