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The Concentration of HCl, a strong acid, is 0.5 mol/L. If 20 mL HCl is needed to titrate 40 mL of NaOH, what is the Concentration of NaOH?

2. What would be the molar concentration of a HCL solution if 25.0 mL of the solution is neutralized by 15.5 mL of 0.800 mol/L NaOH?

3. a) Explain what an equivalence point is in a titration.
b) What is the purpose of an indicator in the solution with the unknown concentration?

4. A strong acid and a weak acid that are both 1.0 mol/L react differently with zinc. Choose two acids and with the aid of equations and dissociation, explain why this is the case.

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Related questions

Please provide the steps for the solution. I am particularly confused with what I'm supposed to subtract the total moles of HCl with. I think the concentration of the solution can be determined via M1V1=M2V2 but not sure

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Ammonia (NH3) is a weak base with a pKb of 4.75. Its conjugate acid, ammonium (NH4+) has a pKa of 9.25. Set up a titration using 20.00 mL of HCL to titrate 20.00 mL of aqueous ammonia solution.

Concentration of HCl soln: 0.1044 mol/L 

Initial buret reading (mL): 0.00

Buret reading at equivalence pt (mL): 14.41

Calculate the following:

a.) Moles of HCl added at equivalence pt

b.) Moles of NH3 in sample

c.) NH3 concentration (mol/L)

d.) pH at equivalence point

e.) pH at half the volume required to reach equivalence

 

Lab Results 1.For your coarse titration record the following results. volume of NaOH solution in the burette at the start (mL) volume of NaOH solution in the burette at the end (mL) volume of NaOH solution dispensed (mL) volume of HCl solution in the flask (mL) Data Analysis 2.Calculate the molarity of the HCl concentration using your coarse titration results. Experiment 2: Perform a Fine Titration Lab Results 1.For your fine titration record the following results. volume of NaOH solution in the burette at the start (mL) volume of NaOH solution in the burette at the end (mL) volume of NaOH solution dispensed (mL) volume of HCl solution in the flask (mL) Data Analysis 2.Calculate the molarity of the HCl concentration using your fine titration results. Conclusions 1.What do you expect to happen if you forget to add phenolphthalein to the Erlenmeyer flask? 2.Suppose you had to titrate a solution of NaOH of unknown concentration with a solution of HCl of known concentration using phenolphthalein as an indicator. How will you determine the color change? 3.Suppose you titrated a sample of acetic acid (monoprotic acid) with a 0.125 M solution of NaOH. Given the data in the table below, what is the concentration of the acetic acid solution? volume of 0.125 M NaOH dispensed 22.40 mL volume of acetic acid solution used 15.00 mL volume of water added to the HCl solution 15.00 mL

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