Calculate the molarity of a solution prepared by dissolving 3.12 grams of gaseous HCL in enough water to make 26.8 mL solutions.
a. 1.6 M HCL
b. 0.8 M HCL
c. 3.2M HCL
d. 5.4 M HCL

Calculate the final pH of 25 mL of buffer 0.1M Tris.HCl/Tris buffer, pH=6.60 after the addition of 1.00mL of 0.1M NaOH. pKa is 8.08.
use the 0.10M Tris.HCl and 0.10M Tris to prepare 100mL, pH=6.6 solution. it calculated by pre-lab, it need 96.8 mL 0.10M Tris.HCl and 3.2mL Tris. and take 25mL pH=6.6 solution, then add 1mL of 0

How many milliliters of 3.00 M hydrochloric acid would be needed to react completely with a milk of magnesia tablet that contains 310 mg of Mg(OH)2? The neutralization reaction produces magnesium chloride, MgCl2, and water.

103897 okay if expalin math Only for above listed OTA-ONLY. All others called in.
Please EXPLAIN the math.
100 mL of a 0.1 M NaOH solution is being titrated with 0.2 M HCl solution.
a) What is the pH of the solution after 25 mL of the HCl solution has been added?
b) What is the solution after an additional 20 mL of HCl solut

1. 10.00 mL of 0.1000 M NH3 was diluted with distilled water to
40.00 mL. Calculate the pH of the dilute solution. (Kb NH3 = 1.8*10^-5)
2. The dilute solution was titrated with 0.0500 M HCl. Write the equation for the reaction between ammonia and hydrochloric acid. Calculate the pH of the solution after adding 4.00 mL

I have four problems that I don't understand how to figure out. I've done problems 16-20 but don't know how to do 21-24.
I've attached the whole page from the exam for the information it provides. I've boxed my previous answers in case they are needed to figure out the four questions.
I need help on the third page. The secon

I am confused on how to calculate the concentratin of the HCl solution -
below are the answers so far that I have to get the final answer -please help. I am stumped on question 2 The concentration of the NaOH is known to be 0.1M
1. For your most exact titration, record the following:
(a) Volume of NaOH solution in