A 2.0 milliliter sample of NaOH solution is exactly
neutralized by 4.0 milliliters of a 3.0M HCI solution.
What is the concentration of the NaOH solution?

Question

A 2.0 milliliter sample of NaOH solution is exactly
neutralized by 4.0 milliliters of a 3.0M HCI solution.
What is the concentration of the NaOH solution?

rogue · Answer

Use the titration equation (I think that's what it's called).$$M_A V_A = M_B V_B$$

anonymous · Answer

i got 6.0M

anonymous · Answer

i did  3.0*4.0=2.0mL

rogue · Answer

Yeah, that's right.

anonymous · Answer

holy shizz ! i tried by my self xD

anonymous · Answer

hey could you help me with this one

anonymous · Answer

How many mL of 0.20 M of hcl is required to neautralize 100. mL of 0.80 M pottasium hyderoxide

rogue · Answer

Same equation.

anonymous · Answer

could you help me set it up

rogue · Answer

It only gets a bit tricky when you have polyprotic acids or compounds with multiply hydroxides.

jfraser · Answer

words of caution, if I may: the titration equation is only usefuons where the acid/base ratio is 1:1. Any other kind of balancetio won't automatically work

rogue · Answer

0.20 M H+ * V = 0.80 M OH * 100 mL

anonymous · Answer

uhm im gettign 40 0r 400

rogue · Answer

Yeah, 400 mL is right.

jfraser · Answer

$$M_{acid}*V_{acid} = M_{base}*V_{base}$$

anonymous · Answer

thanks alot guys :)

anonymous · Answer

What is the molarity of hydrogen ions in a 2.7M solution of the strong acid HCl

rogue · Answer

Strong acids dissociate almost completely. So that 2.7 M of HCl effectively becomes 2.7 M H+ and 2.7 M Cl-.$$HCl \rightarrow H^+ + Cl^-$$