1. (25 pt.) I have a beaker with 250.0 mL of distilled water. I dissolve 10.0 g of sodium acetate (NaOAc) and 10.0 g of potassium cyanate (KCNO). What is the pH of the resulting solution?
They are both salts. I dissociate the NaOAC and I get Na+ and OAc-
I dissociate the KCNO and I get K+ and CNO-
The Na+, K+ are spectators, so I ignore them.
The OAc- and the CNO- form a buffer. If I convert g to moles, I have 0.125 moles of OAC- and 0.177 moles of CNO-
pH=pKa + log (acid/base) = 4.26 + log(0.125/0.177)= 4.11
pH=4.11!
I have a beaker with 250.0 mL of distilled water. I dissolve 10.0 g of sodium nitrite (NaNO2) and 10.0 g of barium nitrite [Ba(NO2)2]. What is the pH of the resulting solution?
1. I have a beaker with 250.0 mL of distilled water. I dissolve 10.0 g of ammonium chloride (NH4Cl) and 10.0 g of methylammonium Chloride (CH3NH3Cl). What is the pH of the resulting solution?
Please help me with this work problem and explain. Determine the pH of the following solutions: a) You dissolve 3.42 g of acetic acid with enough water in a 250.0 ml volumetric flask. Ka = 1.76*10^-5 b) You dissolve 2.64 g of sodium acetate with enough water in a 250.0 ml volumetric flask. c) You mix all solutions A and B from above together into a larger beaker( buffer solution) d) You add 420 ml of 0.75 NaOH into solution...
Table 3: Sodium Acetate Data Sodium Acetate (g) Molarity of Sodium Acetate (Step 7) 4.0 g 0.4876 M Table 4: Buffer Solutions and pH Readings for Beakers A, B, C, D, and E Buffer mL of Acetic Acid mL of Sodium Acetate pH measured A 5 5 4.3 B 5 1 3.6 C 10 1 3.4 D 1 10 5.3 E 1 5 5.0 Post-Lab Questions What are the calculated pH values for the buffers (A,B,C,D and E) that you...
Determine the pH of the following solutions a) You dissolve 2.75 g of acetic acid with enough water in a 500.0 mL volumetric flask. Ka of acetic acid = 1.76 x 10−5 b) You dissolve 3.20 g of sodium acetate with enough water in a 500.0 mL volumetric flask. c) You mix all of Solution A and B from above together into a larger beaker d) You add 3.50 mL of 1.0 M HCl into Solution C (buffer)
what will the ph be for solution Q??
PROCEDURE The pH meter should already be calibrated at pH 4, 7 and 10. If your pH meter appears not to be operating properly, notify your TA and they will recalibrate the meter. Please handle the pH probe carefully; the tip is made of a fragile glass membrane. Be sure to rinse the probe with DI water and blot it dry with a Kimwipe whenever it is transferred from one solution to...
volume 20 distilled 20 acetic HCL 20 20 NaOAc 20 naoh solution A 20 predict ph 7 4 .2 1 9 12 10.00 ml of 7 0.2 acetic acid and 10.00 ml 0.2 m sodium acetate
What is the new expected pH level for each question. 20 ml of sodium hydroxide solution added 25 ml of sodium hydroxide solution added Bonus/ Extra credit: Determine the pH of the resulting solution that is formed when 20.0 ml of 0.05 Molar NaOH is added to 10.0 ml 0.20 molar acetic acid/sodium acetate solution. (Hint: a 0.20 molar acetic acid/sodium acetate means that the buffer contains 0.20 molar acetic acid and 0.20 molar sodium acetate solutions combined).
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...
A solution of sodium was prepared by dissolving 0.0309 g of NaCl in distilled deionized water and brought up to the mark in a 200 mL volumetric flask. 10.0 mL of this solution was diluted to 250.0 mL. What is the concentration (ppm) of sodium the final solution