So... what's the question?
3.00 M
The HCL concentration is 1.2M or 1.2N
Aqueous titration: the ion to be titrated is in an aqueous solution Nonaqueous titration: the ion to be titrated is in an nonaqueous solution
0.289 Moles is the molarity of an NaOH solution if 4.37 ml is titrated by 11.1 ml of 0.0904m hno3.
Tytrate or Analyte
3.00 M
Mass of H2O2 = 0.637 g
A solution that has been titrated against a primary standard solution.
The HCL concentration is 1.2M or 1.2N
Aqueous titration: the ion to be titrated is in an aqueous solution Nonaqueous titration: the ion to be titrated is in an nonaqueous solution
0.289 Moles is the molarity of an NaOH solution if 4.37 ml is titrated by 11.1 ml of 0.0904m hno3.
Tytrate or Analyte
basic
You need to know the volume of the weak acid being titrated so you can find how many moles of base are needed to match that of the acid.
I don't know, I suppose we have to ask a chemist.
In an acid-base titration problem, the formula to use is: MaVa = MbVb, where the molarity of the acid times its volume equals the molarity of the base times its volume.Here, we have:Ma(10.00mL) = (0.135M)(31.25mL)Solving for Ma = 4.22M.mL / 10.00mL = 0.422M(Note: This is only valid for monoprotic acid with monoprotic bases only, as in this case. If it were titrated with 0.135M carbonate (CO32-) the findings need to be doubled.)
(25.00ml HBr)( Molarity ) = ( 18.80ml NaOH )( 0.150 M ) Molar concetration of HBr = 0.108 M