- log(0.000626 M H2SO4) = 3.2 pH -----------
You need 49,8 mL H2SO4 6,4M.
(25.00ml H2SO4)(H2SO4 M) = (22.65ml NaOH)(0.550M) = 0.4983M H2SO4
14.1 mL is required to titrate 10.00 ml of 0.526 M H2SO4.
0.08 n
- log(0.000626 M H2SO4) = 3.2 pH -----------
You need 49,8 mL H2SO4 6,4M.
(25.00ml H2SO4)(H2SO4 M) = (22.65ml NaOH)(0.550M) = 0.4983M H2SO4
14.1 mL is required to titrate 10.00 ml of 0.526 M H2SO4.
how will make solution for 0.005 h2so4
0.08 n
The first solution is more concentrated because it contains 6 moles of H2SO4 per one liter of solution. The second solution is less concentrated because it contains 0.1 moles of H2SO4 in one liter. In equal amounts of each example, the first would have more H2SO4.
Using V * M = constant at dilution = amount of H2SO4 [mol] in both of the solutionsV= volume [L] of the solutionM= molarity [mol/L] of the solutionSo: V *18.0 = 24.9 * 0.195 gives V = ( 24.9 * 0.195 ) / 18.0 = 0.270 L
H2SO4 is not metals. These two can go together and make H2.
Molarity = moles of solute/volume of solution 0.324 M H2SO4 = moles H2SO4/500 ml 162 millimoles, or, more precisely to the question 0.162 moles H2SO4
30 mL water.
100 cm make 1 meter. Answer is 45 meters