# CHEM HELPP!!!

posted by .

Imagine that you are in chemistry lab and need to make 1.00 of a solution with a pH of 2.50.
You have in front of you

100 of 7.00×10−2 , HCL
100 of 5.00×10−2 , and NaOH
plenty of distilled water.

You start to add HCL to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH . Once you realize your error, you assess the situation. You have 81.0 ml of HCl and 90.0ml of NaOH left in their original containers.

Assuming the final solution will be diluted to 1.00L, how much more HCl should you add to achieve the desired pH?

• CHEM HELPP!!! -

pH=log(H)
2=log H
H=1E-2=.01M

HCl net must be .01moles.

You have .009*7E-2 moles or .009*.063 moles

So additional moles must be .01-above.

check my thinking.

• CHEM HELPP!!! -

your answer is pretty cracked out, if you gona help, show your steps and help

## Similar Questions

1. ### chem

HCl is a strong acid and ionizes 100%. NaOH is a strong base and ionizes 100%. We have no way of knowing the pH of HCl + H2O because the problem doesn't state the amount of HCl added or the concentration of HCl. For the NaOH + HCl …
2. ### Chemistry

Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.70. You have in front of you * 100 mL of 6.00×10−2 M HCl, * 100 mL of 5.00×10−2 M NaOH, and plenty of distilled water. You start …
3. ### chemistry- some help plzz totally lost on this one

Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.70. You have in front of you * 100 mL of 7.00×10−2 M HCl * 100 mL of 5.00×10−2 M NaOH, and * plenty of distilled water. You start …
4. ### CHEMISTRY HELP!

(1) A beaker with 165 mL of an acetic acid buffer with a pH of 5.00 is sitting on a bench top. The total molarity of the acid and conjugate base in the buffer is 0.100M. A student adds 7.20mL of a 0.320M HCl solution to the beaker. …
5. ### Chemistry Help! Thank you :)

Assuming the final solution will be diluted to 1.00 , how much more should you add to achieve the desired pH?
6. ### Science

25 cm of 1.0 mol dm− NaOH is added to 25 cm of 1.0 mol dm− HCl. The temperature rise is 6¢XC. Which reactants will also give a temperature rise of 6¢XC?
7. ### Chemistry

1.What mass of NaOH(s) must be added to 300 mL of HCl 0.25 M in order to completely neutralize this acid?
8. ### Chem

Calculate ΔG at 25°C for the precipitation of lead(II) chloride from mixing 100. mL of 0.025 M lead(II) nitrate solution with 100. mL of 0.15 M sodium chloride solution. The ΔG° for the reaction at 25°C = −27.36 …
9. ### chemistry

So I did a titration lab at school with NaOH and HCl. i have to find: - volume used, NaOH - Moles of NaOH - Moles of HCl -Volume used unknown HCl - Molarity of HCl solution My concentration of NaOH stock solution was 0.100 mol/lL Final …
10. ### Chemistry (molarity) (sorta an emergency)

I'm doing a titration lab and writing a lab report where I'm sort of stuck on how exactly to find the concentration of HCl. These are the following info I have from the lab, Equation: HCl(aq)+NaOH(aq)-> H2O(l)+NaCl(aq) -Calculated …

More Similar Questions