# Chemistry

I have troubles with a titration of NaOH and HCl.

The volume of the HCl is 30 ml and its concentration is 0.1 mol per liter
The volume of the NaOH is 25 ml and the concentration is to be worked out. I understand that the reaction ratio for HCl to neutralize NaOH is 1:1.
But does that mean that 0.1 mol of HCl have to react with 0.1 mol of NaOH??? Can someone help me, PLEASE......

1. 👍 0
2. 👎 0
3. 👁 106
1. Yes, the ratio is 1:1 because of the equation.
HCl + NaOH ==> NaCl + H2O

It means 0.1 mol HCl and 0.1 mol NaOH react exactly; also it means that the moles NaOH must equal the moles of HCl at the equivalence point.
So if you started with 30 mL of 0.1 HCl, you started with M x L = 0.030L x 0.1 M = 0.003 moles HCl. Therefore, at the equivalence point, you must have added 0.003 mole NaOH. Since M = moles/L, 0.003/0.025 (the volume of NaOH) = 0.12 M for the NaOH. For titrations that are 1:1, it is simpler to use mL x M = mL x M
30 x 0.1 = 25 x M and solve for the unknown M.

1. 👍 0
2. 👎 0
2. Thanks!

1. 👍 0
2. 👎 0
posted by Jazz
3. m1v1=m2v2

1. 👍 0
2. 👎 0

## Similar Questions

1. ### 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

asked by Ray on November 13, 2016
2. ### chemistry

HCl is titrated with NaOH. When doing the titration, some of the NaOH splashed onto the inside surface of the Erlenmyer flask, and you forgot to rinse it into your sample. Would the systematic error be falsely high, low, or

asked by bria on September 17, 2006
3. ### 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

asked by julie on January 4, 2015
4. ### chemistry

The titration of HCl with NaOH is represented by the equation HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) What volume of 0.100 M HCl is required to titrate 50.0 mL of 0.500 M NaOH?

asked by kathy on December 6, 2011
5. ### chemistry

Question about titration calculations in analysis of antacids lab. We did a lab yesterday with antacids, HCl and NaOH and I'm having trouble doing the calculations. The information known is the following: 1)0.10M NaOH 2)0.10M HCl

asked by Mindy on March 11, 2010
6. ### Chemistry

A titration setup was used to determine the unknown molar concentration of a solution of NaOH. A .025 M HCl solution was used as the titration standard. The following data were collected. Trial 1 Trial 2 Trial 3 Initial NaOH Buret

asked by Anonymous on December 9, 2018
7. ### chemistry

Hello. In the class, we did the experiment to calculate the value of Kc for the following reaction: CH3COOH+CH3CH2OH ÌCH3COOCH2CH3+H2O we measured the mass for 5 cm^3 of all 5 compound above: CH3COOH 5.236 g CH3CH2OH 4.021 g

asked by masaya on November 1, 2008
8. ### Chemistry - Acid Base Titration

When you complete a acid base titration of NaOH and HCl and how to you find the molarity/concentration of HCl. I used 9 mL of HCl with 50 mL of water. But when solving for concentration, do I use 9 mL or 59 mL (water + HCl)? Also,

asked by Steve on January 31, 2008
9. ### Chemistry - Solubility

INFORMATION: [HCl] = 0.1388 M We placed 0.5 g Ca(OH)2 in 100 mL of the following solutions: A 25 ml aliquot was used Flask A: Distilled Water (7.4 mL of HCl needed to titrate) Flask B: 0.05 M NaOH (7.5 mL of HCl needed to titrate)