How much NaOH is needed to prepare 576 mL of solution with a pH 10?

Is it possible to calculate concentration of a solution, OH- concentration, and H+ concentration from just a pH given (no specific base or acid)?

Is the concentration of a solution the same as the concentration of [OH-] or [H+]?

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No it is not. The fixed pH solutions only work with weak acids or bases and their conjugate salts.

pH ten means the -log of the activity of the hydrogen ion against a standard calomel electrode is 10.
Even electrodes are standardized against buffer solutions.

This also means the concentration of hydrogen ion is at 10^(-10) M for this solution. The hydroxide concentration would have to be at 14-10 =4 =pOH or 10^(-4) M

That is ...

Solution Summary

The question is answered step-by-step with short explanations throughout.

I have a big Chemistry test Friday, and I have to learn how to find the average molarity of NaOH (0.1 M) from three trial titration experiments I did in lab.
Titration #1
Volume of NaOH used =3.9 ml
Titration #2
Volume of NaOH used = 3.9 ml
Titration #3
Volume of NaOH used = 4.0 ml.........AVERAGE MOLARITY OF NaOH___

Please show steps and provide a short explanation.
The formula weight of NaOH is 40.0.
1. How many grams of NaOH are needed to make 1M solution?
2. How many grams of NaOH are needed to make a 0.5M solution?
3. How many grams of NaOH are needed to make 0.25M solution?
4. How many grams of NaOH are needed to make 500m

I am a bit stumped with the following word problems, and am having trouble setting up the appropriate equations. If anyone can guide me in the right direction, or suggest ways on how to set up the right equations, I would greatly appreciate it:
1) Calculate the weight of 50% NaOHsolution required to prepare 500 ml of 0.1 M N

How many millimeters of 0.500 M NaOH should be added to 10.0 g of tris hydrochloride to give a pH of 7.60 in a final volume of 0.250 mL?
Useful information: Tris hyrochloride fw = 157.596 g/ml
The Kb for tris is 1.2 x 10^-6
You can represent tris hydrochloride as BH+ and its conjugate base, tris, as B.

Write a balanced equation for the neutralization of acetic acid with NaOH.
I have actually gotten better at balancing equations---but I have no idea where to even start with this one.
Any help you can provide would be greatly appreciated.
Thank You,

Boric acid, H3BO3, is found in some laundry detergents, antimicrobials, and pesticides. With a Ka = 5.8 x 10^-10 it is a weak acid that behaves as a monoprotic acid. Assume you titrate 20.0 mL of 0.11 M boric acid with 0.100 M NaOH. (Show work)
1. Write the equation:
2. What is the pH of the solution before titration begin

I'm wondering if you could help me answer a few questions about a lab I'm doing. We are preparing an a,b-unsaturated ketone via Michael and aldol condensation reactions. The reactants are trans-chalcone and ethyl acetoacetate (in ethanol and NaOH). This creates 6-ethoxycarbonyl-3,5-diphenyl-2-cyclohexenone.
1) A white so

For your most exact titration, record the following:
(a) Volume of NaOHsolution in the burette at the start (mL): The volume of NaOHsolution in the burette at the start was 50 mL.
(b) Volume of NaOHsolution in the burette at the end (mL): The volume of NaOHsolution in the burette at the end was 33.65 mL.
(c) Volume