![measured pH = cal, pKa = q. I 0 pH1 after 5 drops of NaOH-14- pH after 5 drops of HCl = gng BE SURE TO GET T 3) Buffer System with 2 ml acid + 20 ml conjugate base [B]/ [HB] = 10 BE SURE TO GET THIS CORRECT!! (use H+H Eq. above to calculate pKa) measured pH- 450 pH after addition of XS NaOH-10.00 dition of XS NaOH = calculated Ka - calculated. pKa = Show Calculation below leg 6,S](http://img.homeworklib.com/questions/53a98450-0c49-11ec-99c8-ff67b571b6f3.png?x-oss-process=image/resize,w_560)
Homework Answers
pH = 9.5
[B] / [HB] = 10 = [conjugate base / acid ]
pH = pKa + log [conjugate base / acid ]
9.50 = pKa + log 10
8.50 = pKa + 1
pKa = 8.50
pKa = -logKa
Ka = 10^-pKa
Ka = 10^-8.50
Ka = 3.16 x 10^-9
so
Ka = 3.16 x 10^-9
pKa = 8.50
Add Answer to:
Calculate the pka and ka given the pH.
Please show ALL steps
measured pH = cal,...
i need to find the ratio of B- and HB to create a ph level of...
i
need to find the ratio of B- and HB to create a ph level of 11
using the pka found in part 1 and 2 of question c. what equation
would i use to fibd the ratio and the volume?
5. Preparation of Buffer Target pH to be prepared pK, from C.1 and C.2 Show calculation of B)/(HB) ratio needed: Ratio [B]/[HB) needed: Volumes used to create above ratio: ml. HB ml phl of prepared buffer c. Some Properties...
1) Find the Difference between measured pH and calculated theoretical pH of solutions 1-6 for [HC2H3O2]...
1) Find the Difference between measured pH and calculated
theoretical pH of solutions 1-6 for
[HC2H3O2] (M) and
[C2H3O2−] (M)
2) Find the Difference between measured pH and calculated
theoretical pH of solutions 1-6.
3) In this experiment, we define the buffer capacity of a buffer
as the number of drops of either 3.0 M HCl or 3.0 M NaOH needed
before the pH of the solution changes by more than 0.5 pH units.
For example, if the pH of...
3. Calculate the pH (Ka = 2.0 x 10-2 alculate the pH at the beginning of...
3. Calculate the pH (Ka = 2.0 x 10-2 alculate the pH at the beginning of a titration of 50.00 of 0. 20 x 10-2) with NaOH solution. If the quadratic equa e accurate, what would the percent error in the pH if the simple equation were used to calculate the phine of 50.00 of 0.005M HA quadratic equation is assumed to the simpler (square root) 4. According to Figure 19.1 at which point(s) ABCD on the titration curve does...
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 conju...
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 ×...
In a titration, 10.00 mL of .1000M butanoic acid, CH3CH2CH2COOH (Ka = 1.54 * 10^-5), is...
In a titration, 10.00 mL of .1000M butanoic acid, CH3CH2CH2COOH (Ka = 1.54 * 10^-5), is titrated with .1000M NaOH (aq). a. Calculate the pH of the system when 10.00 mL of NaOH (aq) has been added. Use ICF/ICE tables to support your answer. b. Sketch the general shape of the titration curve for this system. Be sure to label the axes, any buffer regions, the point at which pH = pKa and the equivalence point. You do not need...
Question 2: A) Calculate the pH of the buffer that results from mixing 56.1 mL of...
Question 2: A) Calculate the pH of the buffer that results from mixing 56.1 mL of a 0.406 M solution of HCHO2 and 11.9 mL of a 0.606 M solution of NaCHO2. The Ka value for HCHO2 is 1.8×10−4 B) Calculate the initial pH and the final pH after adding 0.010 mol of NaOH. 300.0 mL of a buffer solution that is 0.225 M in HCHO2 and 0.280 M in KCHO2 C) Calculate the initial pH and the final pH...
Please help, I'm so confused!!!! This is due wednesday night!!! i'm gonna fail :(((( pH of...
Please help, I'm so confused!!!! This is due wednesday night!!!
i'm gonna fail :((((
pH of Buffer Solutions Procedure: Acetic Acid-Sodium Acetate Buffer (pKa acetic acid = 4.75) Weigh about 3.5 g of Na2C2H302 3H2O, record the exact mass, and add to a 250 ml beaker. Measure exactly 8.8 mL of 3.0 M acetic acid (use 10 mL grad cylinder) and add to the beaker containing the sodium acetate. • Measure exactly 55.6 mL of distilled water and add to...
1) Calculate the pH of the 1L buffer composed of 500 mL of 0.60 M acetic...
1) Calculate the pH of the 1L buffer composed of 500 mL of 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of HCl is added (Ka HC2H3O2 = 1.75 x 10-5). Report your answer to the hundredths place. 2) Calculate the pH of the 1L buffer composed of 500 mL 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of NaOH is added (Ka HC2H3O2 = 1.75...
how do the measured ad calculated pHs differ? and how do I calculate the pHs? the...
how do the measured ad calculated pHs differ? and how
do I calculate the pHs?
the volume of the 3M HOAc added is 8.8mL
Experiment Part B: Buffer Capacity Mass NaOAC-3H0_3.5 -g Volume of 3.0 M HOAc added mL Solution Calculated pH Buffer Solution 6.0 M HCI - log (16) Measured pH 9.91 28 13.72 4.43 5.28 -.78 14.78 6.0 M NaOH 14 - (-.78) Buffer + HCI Buffer + NaOH H0+ HCI 1,0 + NaOH I 1.2 12.69 Show...
Please explain to me how I solve this Calculate the pH of a 0.2 M acetate...
Please explain to me how I solve this
Calculate the pH of a 0.2 M acetate buffer (pKa = 4.77) that contains twice as much acid as conjugate base. Calculate the pH of the solution that results following the addition of 10mL of 1M NaOH to 40mL of 1M NH_4C1 Ka = 5.62 times 10^-10
i
need to find the ratio of B- and HB to create a ph level of 11
using the pka found in part 1 and 2 of question c. what equation
would i use to fibd the ratio and the volume?
5. Preparation of Buffer Target pH to be prepared pK, from C.1 and C.2 Show calculation of B)/(HB) ratio needed: Ratio [B]/[HB) needed: Volumes used to create above ratio: ml. HB ml phl of prepared buffer c. Some Properties...
1) Find the Difference between measured pH and calculated
theoretical pH of solutions 1-6 for
[HC2H3O2] (M) and
[C2H3O2−] (M)
2) Find the Difference between measured pH and calculated
theoretical pH of solutions 1-6.
3) In this experiment, we define the buffer capacity of a buffer
as the number of drops of either 3.0 M HCl or 3.0 M NaOH needed
before the pH of the solution changes by more than 0.5 pH units.
For example, if the pH of...
3. Calculate the pH (Ka = 2.0 x 10-2 alculate the pH at the beginning of a titration of 50.00 of 0. 20 x 10-2) with NaOH solution. If the quadratic equa e accurate, what would the percent error in the pH if the simple equation were used to calculate the phine of 50.00 of 0.005M HA quadratic equation is assumed to the simpler (square root) 4. According to Figure 19.1 at which point(s) ABCD on the titration curve does...
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 ×...
Please help, I'm so confused!!!! This is due wednesday night!!!
i'm gonna fail :((((
pH of Buffer Solutions Procedure: Acetic Acid-Sodium Acetate Buffer (pKa acetic acid = 4.75) Weigh about 3.5 g of Na2C2H302 3H2O, record the exact mass, and add to a 250 ml beaker. Measure exactly 8.8 mL of 3.0 M acetic acid (use 10 mL grad cylinder) and add to the beaker containing the sodium acetate. • Measure exactly 55.6 mL of distilled water and add to...
how do the measured ad calculated pHs differ? and how
do I calculate the pHs?
the volume of the 3M HOAc added is 8.8mL
Experiment Part B: Buffer Capacity Mass NaOAC-3H0_3.5 -g Volume of 3.0 M HOAc added mL Solution Calculated pH Buffer Solution 6.0 M HCI - log (16) Measured pH 9.91 28 13.72 4.43 5.28 -.78 14.78 6.0 M NaOH 14 - (-.78) Buffer + HCI Buffer + NaOH H0+ HCI 1,0 + NaOH I 1.2 12.69 Show...
Please explain to me how I solve this
Calculate the pH of a 0.2 M acetate buffer (pKa = 4.77) that contains twice as much acid as conjugate base. Calculate the pH of the solution that results following the addition of 10mL of 1M NaOH to 40mL of 1M NH_4C1 Ka = 5.62 times 10^-10
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