1. I mixed 20 mL of .1M CH3COOH + 20 mL of .1M NaCH3CO
2. I measured out the 10 mL of my buffer into a vial and measured the pH of my buffer solution to be 4.95.
From there does that mean from my 10 mL of buffer, my moles of acid is 1.12x10-5M and my moles of base from 10.0 mL of buffer is 8.91x10-10M?
I got 1.12x10-5M and 8.91x10-10M from this:
And how would I find the Ka value? I thought I would have to do this:
I'm just wondering if these steps are correct.
A buffer is created by combining 325.0 mL of 0.750 M CH3COOH with 225.0 mL of 0.500 M NaCH3COO. (Ka for CH3COOH = 1.76 x 10-5) a)What is the pH of the buffer both before and after the addition of 25.00 mL 1.00 M HCl? b)What volume of 1.75 M NaOH would be required to position the buffer at it's ½ equivalence point (pKa point)? What is the pH of the buffer at this time?
• The large container marked “DI water” • 1 M CH3COOH Record the pH of this solution for later use. (4.76) • 1 M NaCH3COO • Two (2) 600-mL beakers Transfer 20 mL of CH3COOH to one of the empty beakers. Transfer 20 mL of NaCH3COO to the same empty beaker. Add 360 mL of DI water. (400 mL total in the beaker.) Record the pH of this solution for later use (4.76). a. moles of CH3COOH in the buffer...
5. Calculate the grams of NaCH3COO required for 100.0 mL of 0.20 M CH3COOH solution to achieve a pH of 4.40. (Assume no volume change.) K = 1.8 x 10-5 6. What is the pH of 100.0 mL of buffer consisting of 0.20 M CH3COOH/0.20 M NaCH3COO after 10.0 mL of 0.20 M HC1 was added into the solution ? Kg = 1.8 x 10-5 7. The pH of a sodium acetate-acetic acid buffer is 4.80. Calculate the ratio of...
How many grams of NaNO2 should be mixed with 20 mL of 0.5 M HNO2 to buffer it at a pH of 3.50? The Ka for HNO2 is 7.1 x 10-4.
I need the highlighted parts, and check if what I did is correct. Thanks! I. Equilibrium Glacial CH3COOH Final buret reading 46 Moles acetic acid 0.0524 used (show work) Molarity of solution (show work) Initial buret reading 49 0.524 mL acetic acid used 3 mL H30 1eq 1.4125 x 10-3 pH measured 2.85 Using appropriate concentrations, complete the "I", "C", "E" table below [CH3COO- [CH:COОH] 0.524 [H:О"] Initial concentrations +1.4125x10-3 1.4125x10-3 +1.4125x10-3 1.4125x10-3 Change Equilibrium Conc Calculate the value of...
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...
4- Calculate the pH when you add 40 ml 0,1 N CH3COOH onto 20 ml 0,1 N NH3? (Ka:1.75 x 10-5, Kb: 1.8 x 10-5, Khe 10- 14) a) 3.48 b) 5,48 C) 1,48 d) 6.48 4,58
1) 7. 10.0 mL of 0.10 M HBr is mixed with 10.0 mL of 0.10 M HCOOH. What is the pH? 2) 15. Calculate the pH of a solution containing 2.5 x 10 –2 mol of nicotinic acid (a monoprotic acid dissolved in 350 mL of water. ( K a = 1.1 x 10 -5 ) 3) A 1.0 L buffer solution is made up of 0.15M NaF and 0.20 M HF ( pK a = 3.17) . 0.05 mol...
1- 50 ml of a 2 M Na acetate solution is mixed with 100 ml of a 0.1 M of acetic acid solution. Calculate the pH of the buffer. Show your calculation Pk, value of acetic acid = 4.75 (4 points) PH=4.75+ 50x2 - 100 = 10 100001 PH = 4.7 + 10 = 114.75 Describe how you make a 250 ml of a 10% glycine solution (MW=75.07). EXPLAIN the steps that you would take in Lab. 4 points 2-Determine...
i already know they answer please explain your solutions Ka for CH3COOH = 1.8x10^-5 pka i calculated 4.74 ID: A fer- a solut monione blir rw Name: was 11. If 0.40 g of solid NaOH is added to 1.0 liter of a buffer solution that is 0.10 Min CH,COOH and 0.10 Min NaCH,COO, how will the pH of the solution change? a. The pH increases from 4.74 to 4.83. b. The pH decreases from 7.00 to 4.83. c. The pH...