Can someone help me with these chemistry lab questions?
9. It takes 38 mL of 0.75 M KOH solution to completely neutralize 155 mL of a sulfuric acid solution (H2SO4). What is the concentration of the H2SO4 solution?
10. A few small drops of water are left in a buret that is then used to titrate base into an acid solution to determine the concentration of the acid. Will this small amount of water have any effect on the determined value for the concentration of the acid? If so, how is it affected?
11. It takes 12.5 mL of a 0.30 M HCl solution to neutralize 285 mL of NaOH solution. What is the concentration of the NaOH solution?
12. A student carefully pipets 25.0 mL of 0.505 M NaOH into a test tube. She places the test tube into a small beaker to keep it from spilling and then pipets 75.0 mL of 0.305 M HBr into another test tube. Without reading the next steps in her lab manual, the student combines the contents of both test tubes in her beaker. Is the solution formed from the contents of the two test tubes acidic or basic? What is the pH of the resulting solution?
- Roger the MoleLv 74 weeks agoFavorite Answer
H2SO4 + 2 KOH → K2SO4 + 2 H2O
(38 mL) x (0.75 M KOH) x (1 mol H2SO4 / 2 mol KOH) / (155 mL H2SO4)=
0.092 M H2SO4