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?
pH=pKa+log(b/a)
pH=4.77+ log(10/68.99)/(10/229.35) = 4.31
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?
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...
is the pH and pOH of the acid solution with [H'] = 0.38 M? What is the [H30") and TOH concentration of an acid solution with pH = 5.5? 3. How many liters of 0.186 M of NaOH(aq) contain 0.135 mol of NaOH? If 0.123 g NaOH is dissolved in enough water to make 250.0 mL of solution, what is the molarity (M) of the sodium hydroxide solution? If 2.00 mL of 0.456 M NaOH is diluted to exactly 100...
You need to produce a buffer with pH = 4.20 by dissolving a weighed amount of sodium nitrate (NaNO2) in 500-mL of 0.65-M benzoic acid (a) What mass of sodium nitrite is required? (Sodium nitrite has a molar mass of 69.00 g/mol). (b) What is the resulting pH if 45-mL of 0.18-M HCl is added to 250 mL your buffer?
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
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)
How many grams of barium nitrite, Ba(NO2)2 would you need in 375 L of solution to have a pH of 8.11? Assume it is completely soluble.
Maps 1. What is the pH of a 0.35 mol/L solution of acetylsalicylic acid (C9H804)? 2 points Your answer 2. What is the pH of a 1.50 mol/L solution of ammonium chloride (NH4Cl)? 2 points Your answer 4 points 3. What is the pH of the buffer resulting of the mixing of 34.4 g of sodium dihydrogen phosphate (NaH2PO4) and 48.5 g of sodium hydrogen phosphate (Na2HPO4) in 2.5 L of distilled water? Your answer 4. What is the pH...
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...