If it takes 35.0 ml of 0.250 m fe2+ to titrate 100 ml of a solution containing cr2o72-, what is the molar concentration of cr2o72-?

0.0146 M

Explanation:

The relevant chemical reaction equation is as follows:

Cr₂O₇²⁻ + 6Fe²⁺ + 14H⁺ ⇒ 2Cr³⁺ +6Fe³⁺ + 7H₂O

In order to find the concentration of Cr₂O₇²⁻, the number of moles of Cr₂O₇²⁻ in the solution must be found. This can be found by relating it to the number of moles of the analyte (Fe²⁺), which can be calculated as follows:

(35.0 mL)(0.250mol/L) = 8.75 mmol Fe²⁺

This is the amount of Fe²⁺ required to react with all of the Cr₂O₇²⁻ present.The moles of Fe²⁺ and Cr₂O₇²⁻ in the reaction are related as follows:

8.75 mmol Fe²⁺ x (Cr₂O₇²⁻ / 6Fe²⁺) = 1.4583...mmol Cr₂O₇²⁻

The concentration of the Cr₂O₇²⁻ solution is then calculated as follows:

(1.4583...mmol) / 100mL = 0.146 mol/L = 0.146 M

a: 45.9 meters

b: 4.29 seconds

step-by-step explanation:

a: h(t)=1/2(-9.8)(3)^2+0(3)+90

h(t)=-4.9(3)^2+90

h(t)=-44.1+90

h(t)=45.9 meters

b: 0=1/2(-9.8)(t^2)+0t+90

0=-4.9t^2+90

-90=-4.9t^2

18.37=t^2

t=4.29 seconds

in the second question, the numbers aren't exact, but they're a close approximation.