chemistry 1st year, for midterm help
posted by ur class fella .
Can any1 help with theses questions. I need to solve these because there will be similar questions on the midterm for me, coming week. Btw I have tried few.
1. How many milliliters of a 15.0%, by mass solution of KOH (Aq) ( d= 1.14g/mL ) are required to produce 27.0 of a solution with pH= 11.45?
Answer is required in mL. Liters is just as fine as mL :P
50.00 mL of 1.45×10−2 M HI(aq) is mixed with 85.00 mL of 1.10×10−2 M KOH (aq).
Above is the data given which is required to solve Q2:
Q2:- What is the of the final solution?
Q3:- What is the pH of an aqueous solution that is 0.124 M NH4Cl?
Thanks in Advance for answering the questions, plz provide the solution if possible?
We will be happy to critique your work, or thinking. We aren't going to do your tests for you.
But these questions were never taught in the class and they are appearing on the mid-term.
ok, here is the thing. I have tried other questions and got the right answer :P
But for question # 2 I convert the ph to pOH and den find the OH-
den I find the # of moles from 6.8% ammonia and den I use the Kb value of ammonia to find the OH- in the 6.8% ammonia and using dat concentration I use the formula c1v1=c2v2 to get the volume which will be required to dilute the 0.625L of pH=11.65?
But I am getting an answer of 334mL which I am told is WRONG.
So plz can some1 tell me what am I missing or doing wrong.
PIEASE TELL ME HOW MANY MAKES THE QUESTION