Chemistry
Turns out all the values were right such as .02505 M and 35.45 g Cl etc, I just didn't need to multiply by 1000 and leave it in grams as you said.
Chemistry
To illustrate the calculation, assume that 21.95 mL of a thiosulfate solution is required to reduce the iodine liberated by 20.85 mL of 0.0200M KIO3 and that 18.63 mL of the same thiosulfate solution reacts with the iodine replaced by 20.00 mL of an unknown solution of sodium ...
Chemistry
Which of the following result in buffered solutions when equal volumes of the two solutions are mixed? a.) .1 M HCl and .1 M NH4Cl b) .1 M HCl and .1 M NH3 c.) .2 HCl and .1 M NH3 d.) .1 M HCl and .2 M NH3 By def. I know that a buffed solution is made from a weak base and it&#...
Chemistry
The question is: what is the ratio [NH3/[NH4+] in an ammonia/ammonium chloride buffer solution with pH= 10.00? (pKa for ammonia=9.25) When working the problem, I tried to solve it a bit backwards, in that I plugged in each of the multiple choices I was given to see which would...
Chemistry
What is the pH of a 0.1 M NaOCl solution (Ka of HOCl is 2.95 x10-8) I did: x squared/.10= 2.95x10-8 x squared= 2.95x10-9 x= 5.43x10-5 -log(5.43x10-5)= 4.27 pH However, the options I'm given are either a.) 3.74 b.) 6.47 c.) 8.23 d.) 10.27 What steps am I doing wrong?
Chemistry
First, the question I'm given is: What is the pH of a 1.0 L solution containing 0.25M acetic acid and 0.75M sodium acetate ( Ka for acetic acid= 1.8x 10-5) So I took the -log(1.8x10-5)= 4.74+log(.75/.25)= 5.22 pH But then I'm asked if .050 mol NaOH is added to the abov...
Chemistry
The indicator bromocresol green (HIn) can be in two different forms: As HIn the color of the indicator is yellow, an In the color of the indicator is blue, and an equilmolar mixture of the two species is green. The Ka of the indicator is 2.5 x 10-5. What is the color of the in...
Chemistry
What is the [H+] of the 0.25 M HCl solution? I'm not given a Ka value, so I'm assuming I won't need one to solve this particular problem?
Chemistry
When looking at a titration curve, I have to determine which is not true and I have it narrowed down to two options: The initial starting point on the titration curve is where pH depends only on [HA]0 or The finial point on a titration curve the pH depends only on [A-] I would...
Chemistry
When the concentration of a weak acid in solution is equal to the concentration of its conjugate base in solution, then: Would pH=pKa or would it equal pH=pKa + 1 like Henderson-Hasselbalch equation?
Pages: 1 | 2 | 3 | 4 | 5 | 6 | 7 | 8 | 9 | 10 | 11 | 12 | 13 | 14 | 15 | Next>>
For Further Reading
