Question

3. Using graphical solution techniques, find the equilibrium pH of the following solutions. Ignore activity corrections...

3. Using graphical solution techniques, find the equilibrium pH of the following solutions. Ignore activity corrections (Note: you will need to find the correct Ka values).

(a) 10-4 M HOCl

(b) 10-4 M NaF

(c) 10-4 M NH4Cl

(d) 10-3 M baking soda (NaHCO3)

(e) 10-3 M baking powder (Na2CO3)

(f) 10-3 M baker’s ammonia ((NH4)2CO3)

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Find the pH for the following solutions: a) A solution that is 0.115 M in HBr...
Find the pH for the following solutions: a) A solution that is 0.115 M in HBr and 0.130 M in HCHO2 b) A 0.25 M CH3NH3I solution? (Kb = 4.4 x 10-4 M for CH3NH2) c) A 0.0180 M solution of HClO2? (Ka = 1.1 x 10-2 M) d) A 0.0180 M solution of Sr(OH)2 e) A 0.170 M solution of KOCl? (For HOCl, Ka = 3.5 x 10-8 M) f) A solution that is 3.00×10−2M in HI and 9.00×10−3M...
A.) Find the pH of a 0.338 M NaF solution. (The Ka of hydrofluoric acid, HF,...
A.) Find the pH of a 0.338 M NaF solution. (The Ka of hydrofluoric acid, HF, is 3.5×10?4.) B.) Determine the [OH?] of a 0.30 M solution of NaHCO3. and Determine the pH of this solution. C.)Find the [OH?] of a 0.46 M  methylamine (CH3NH2) solution. (The value of Kb for methylamine (CH3NH2) is 4.4×10?4.) include units D.) Find the pH of a 0.46? M  methylamine (CH3NH2) solution.
Ignoring activity, how do you determine the equilibrium pH of a solution containing 10^-3 M NH4CL...
Ignoring activity, how do you determine the equilibrium pH of a solution containing 10^-3 M NH4CL (pKa = 9.25) using algebraic techniques? A detailed response please.. not just some expression..
1. Calculate the hydrogen ion concentration, [H+ ], for the two weak acids (pH=-log[H+ ], or...
1. Calculate the hydrogen ion concentration, [H+ ], for the two weak acids (pH=-log[H+ ], or [H+ ]=antilog (-pH). If you have difficulty finding or using the antilog function on your calculator, simply use this: [H+ ]=10-pH . 2. Calculate the hydroxide ion concentration, [OH- ], for the weak base using this formula: pOH=14-pH, then [OH- ]=antilog (-pOH) or [OH-]=10-pOH. 3. Calculate the molar concentrations of the vinegar as well as ammonia. Both are industry standard 5.00% by mass solutions...
1. Which equilibrium is most important in determining the pH of a solution of sodium phosphate?...
1. Which equilibrium is most important in determining the pH of a solution of sodium phosphate? a. HPO42- + H2O = PO43- + H3O+ b. H2PO42- + H2O = H3PO4 + OH- c. H3PO4 + H2O = H2PO4- + H3O+ d. PO43- + H2O = HPO42- + OH- 2. Tina has two aqueous solutions: 1.2 x 10-2 M NaOH and 1.2 x 10-2 M NH3 (KB=1.8x10-5). Which solution has the higher pH? a. the NaOH solution b. the ammonia solution...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT