Consider the reaction: Li₂S(aq) + Co(NO₃)₂(aq) → 2 LiNO₃(aq) + CoS(s) What volume of 0.150 M Li₂S solution is required to completely react with 225 mL of 0.175 M Co(NO₃)₂?

Video transcript

Hey everyone. So here we ask calculate the volume of 0.115 moller of potassium oxide solution. That is need to react with 150 ml of 0.2 molar of Nickel Nitrate. Based on the reaction below recall that polarity. It was the most of the salute. What about leaders of the solution? And since we're given the volume in milliliters here we need to convert from male leaders. Two leaders. We have 1 50 male leaders. We have 1000 mL and one leader. And this will give us 0.15 leaders. So now we can find the moles of potassium oxide. You have 0.15 leaders. We have 0.2 molar of nickel nitrate which is going to be 0. malls of nickel nitrate in one liter. And for every one mole of nickel nitrate we're one more of potassium oxide. And this gives us 0.03 mao of potassium oxide. So now that we have malls are protesting outside and maturity of protecting oxide, we can solve for the volume. Using the maturity equation We have 0.115 smaller Equal to 0.03 laws they bought it by X. Multiply 0.115 caller times X. That equals 0.03 calls. We can solve for X. by dividing both sides by 0.115 forward. So X Equals 0.261 leaders. And since we're giving middle leaders in the question we can convert this from leaders to male leaders. We're gonna have 0.261 leaders. And in one leader we have 1000 their leaders. And this gives us 261 male leaders. Thanks for watching my video and I hope it was helpful.