QUICK CHEM QUESTIONS , PLEASE HELP

[matt123]

The conjugate acid of SeO32- is ??
i thought it would be HseO3- .. is this correct?


is (CH3CH2)2NH a strong or a weak base?

What is the pH of a 1.3M butyric acid solution?? my answer was 2.3

What is the pH of a 2.1M sodium phosphate solution .. kb = 2.1X10^-2. i said 13.3

 Calculate the pH of a buffer made with 0.75M acetic acid and 0.45M sodium acetate. Ka = 1.8 x 10-5.

The pH of a 0.50M solution of a weak base is 11.4. What is the value of Kb for this base?

The pH of a 0.55M solution of hypobromous acid, HOBr, is 4.48. Calculate the value of Ka.


An aqueous solution of ________ will produce a basic solution.
Question 20 answers
   NH4ClO4
   KBr
   NaCl
   NaHSO4
   Na2SO3

thanks in advanced ,
Matt

[Graphite]

The conjugate acid of SeO32- is ??
i thought it would be HseO3- .. is this correct? Yes


is (CH3CH2)2NH a strong or a weak base? Weak

What is the pH of a 1.3M butyric acid solution?? my answer was 2.3 => you need Ka or pKa

What is the pH of a 2.1M sodium phosphate solution .. kb = 2.1X10^-2. i said 13.3 correct

 Calculate the pH of a buffer made with 0.75M acetic acid and 0.45M sodium acetate. Ka = 1.8 x 10-5. => 4.5 use Henderson Hasselbalch equation

The pH of a 0.50M solution of a weak base is 11.4. What is the value of Kb for this base? 7.9E-10

The pH of a 0.55M solution of hypobromous acid, HOBr, is 4.48. Calculate the value of Ka. 1.99E-9


An aqueous solution of [NH4ClO4] will produce a basic solution.
Question 20 answers
   NH4ClO4
   KBr
   NaCl
   NaHSO4
   Na2SO3

thanks in advanced ,
Matt

[matt123]

thanks alot bro

can anyone else please help me with the others?

[matt123]

The conjugate acid of SeO32- is ??
i thought it would be HseO3- .. is this correct? Yes


is (CH3CH2)2NH a strong or a weak base? Weak

What is the pH of a 1.3M butyric acid solution?? my answer was 2.3 => you need Ka or pKa

What is the pH of a 2.1M sodium phosphate solution .. kb = 2.1X10^-2. i said 13.3 correct

 Calculate the pH of a buffer made with 0.75M acetic acid and 0.45M sodium acetate. Ka = 1.8 x 10-5. => 4.5 use Henderson Hasselbalch equation

The pH of a 0.50M solution of a weak base is 11.4. What is the value of Kb for this base? 7.9E-10

The pH of a 0.55M solution of hypobromous acid, HOBr, is 4.48. Calculate the value of Ka. 1.99E-9


An aqueous solution of [NH4ClO4] will produce a basic solution.
Question 20 answers
   NH4ClO4
   KBr
   NaCl
   NaHSO4
   Na2SO3

thanks in advanced ,
Matt

graphite could u please explain the answer to the question u got involving Henderson Hasselbalch equation?

thanks alot bro

[jasoN-]

Calculate the pH of a buffer made with 0.75M acetic acid and 0.45M sodium acetate. Ka = 1.8 x 10-5.



Henderson Hasselbalch equation
b is the [base], a is the [acid]