Anonymous
Anonymous asked in Science & MathematicsChemistry · 9 years ago

Acid-Base Titration, Pre Lab?

1. You perform an acid-base titration to standardize an HCl solution by placing 75.00mL of HCl(aq) in a flask with a few drops of indicator solution. You put 0.1139 M NaOH(aq) into the burette, and the initial reading is 1.51 mL. At the end point (ie, when the solution just turns faint pink), the burette reading is 39.11ml. What is the concentration of the HCl(aq) solution?

2. What volume of 0.0998 M Ba(OH)2 solution standardize in the problem 1, above?

3. Sodium hydrogen carbonate, NaHCO3 (sometimes referred to as bicarbonate) is often sprayed over spilled acid solutions. Write a chemical equation and net ionic equation for the reaction that would take place?

Im in engineering in university, we have to take one chemistry course and its giving me alot of trouble, help is appreciated!!!

Relevance
• Colin
Lv 7
9 years ago

1. Because the reaction is

NaOH + HCl ---> NaCl + H2O

you can use M1 x V1 = M2 x V2 [1:1 relationship]

Amount of NaOH used = 39.11 -1.51 mml = V1

M1 = 0.1139

V2 = 75.00 ml

M2 = what you are trying to find

2. Reaction is Ba(OH)2 + 2HCl ---> BaCl2 + 2H2O

Now you have a 1:2 relationship

so moles of Ba(OH)2 / moles of HCl = 1/2 = vol x molarity Ba(OH)2 / vol x molarity HCl.

Substitute data and solve as before

3. Sodium hydrogen carbonate, NaHCO3 (sometimes referred to as bicarbonate) is often sprayed over spilled acid solutions. Write a chemical equation and net ionic equation for the reaction that would take place?

NaHCO3 + HCl ---> NaCl + H2O + CO2

HCO3- + H+ -----> H2O + CO2

Source(s): retired chem examiner
• Anonymous
4 years ago

interior the lab that I artwork in, we receive samples to objective for their content textile of ammonia. We verify it doing an acid/base titration with standardized H2SO4 the learning is utilized by employing engineers to alter the residences of the catalysts being designed.