Consider the reaction: Li 2 S(aq) + Co(NO 3 ) 2 (aq) → 2 LiNO 3 (aq) + CoS(s) What volume of 0.150 M Li 2 S solution is required to completely react with 225 mL of 0.175 M Co(NO 3 ) 2 ?

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.

Ch.5 - Introduction to Solutions and Aqueous Solutions

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Tro 6th Edition

Ch.5 - Introduction to Solutions and Aqueous Solutions

Problem 42

Chapter 5, Problem 42

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?

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Identify the balanced chemical equation: Li_2S(aq) + Co(NO_3)_2(aq) \rightarrow 2 LiNO_3(aq) + CoS(s).

Determine the stoichiometry of the reaction: 1 mole of Li_2S reacts with 1 mole of Co(NO_3)_2.

Calculate the moles of Co(NO_3)_2 using its concentration and volume: \text{moles of Co(NO}_3\text{)}_2 = 0.175 \text{ M} \times 0.225 \text{ L}.

Use the stoichiometry of the reaction to find the moles of Li_2S needed: \text{moles of Li}_2\text{S} = \text{moles of Co(NO}_3\text{)}_2.

Calculate the volume of 0.150 M Li_2S solution required using the moles of Li_2S: \text{Volume of Li}_2\text{S} = \frac{\text{moles of Li}_2\text{S}}{0.150 \text{ M}}.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced equation. It involves using mole ratios derived from the coefficients of the balanced equation to determine how much of one substance is needed to react with another. In this case, understanding the stoichiometric relationship between Li2S and Co(NO3)2 is essential to find the required volume of Li2S solution.

Molarity

Molarity (M) is a measure of concentration defined as the number of moles of solute per liter of solution. It is crucial for determining how much of a substance is present in a given volume of solution. In this problem, the molarity of both Li2S and Co(NO3)2 solutions is provided, which allows for the calculation of the moles of each reactant involved in the reaction.

Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reactant is essential for calculating how much of the other reactants are needed. In this scenario, determining whether Li2S or Co(NO3)2 is the limiting reactant will influence the volume of Li2S solution required for the reaction.

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Textbook Question

A 55.0-mL sample of a 0.102 M potassium sulfate solution is mixed with 35.0 mL of a 0.114 M lead(II) acetate solution and this precipitation reaction occurs: K₂SO₄(aq) + Pb(C₂H₃O₂)₂(aq) → 2 KC₂H₃O₂(aq) + PbSO₄(s) The solid PbSO₄ is collected, dried, and found to have a mass of 1.01 g. Determine the limiting reactant, theoretical yield, percent yield.

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?

Verified Solution

Key Concepts

Stoichiometry

Molarity

Limiting Reactant

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?