Find the mass of barium metal (in grams) that must react with O 2 to produce enough barium oxide to prepare 1.0 L of a 0.10 M solution of OH - .

Hi everyone. So we have Australian metal reacting with oxygen gas And strontium oxide is produced or asked how many grams of uranium metal is required to produce enough strontium oxide to make 2.1 l Of a 0.5 molar hydroxide ion solution. We're gonna have strange metal which is as our solid Plus auction gas which is 0.2. Yes, this year's trainee um oxide which is S. R. O. Solid. It's a balance is we're gonna put a tour from Australia and it took us from Australia outside. And then we also have standing outside. We're acting with water. The british training hydroxide and for the concentration of O. H minus It's going to be equal to two house construction Australia hydroxide. And so now we need to determine the moles of straining oxide. We have 2.1 leaders, a strong hydroxide And we have 0.5 Mueller of hydroxide solution. They're gonna have 0.5 malls of strontium hydroxide and one leader We have two moles. Australian hijack side Which also has two moles Australian oxide Because they're in a 1-1 ratio. This is just 1.05 Australian oxide. So now that we have moles Australian oxide, you can't convert to grams Australian oxide. We have 1.05 balls Australian oxide. And for two moles Australian oxide, We have two malls Australia. And in one mall Australian We have 87.62 grams of Australia 92 grams. 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 91

Chapter 5, Problem 91

Find the mass of barium metal (in grams) that must react with O₂ to produce enough barium oxide to prepare 1.0 L of a 0.10 M solution of OH^-.

Verified step by step guidance

Write the balanced chemical equation for the reaction: 2Ba + O_2 \rightarrow 2BaO.

Determine the moles of OH^- needed: Use the formula \text{Molarity} = \frac{\text{moles of solute}}{\text{volume of solution in liters}} to find the moles of OH^- required for 1.0 L of a 0.10 M solution.

Relate moles of OH^- to moles of BaO: Since BaO reacts with water to form Ba(OH)_2, and each BaO produces two OH^-, calculate the moles of BaO needed.

Relate moles of BaO to moles of Ba: From the balanced equation, 1 mole of BaO is produced from 1 mole of Ba.

Calculate the mass of Ba: Use the molar mass of Ba to convert moles of Ba to grams.

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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. It involves using balanced chemical equations to determine the relationships between the amounts of substances consumed and produced. In this case, stoichiometry will help us find the mass of barium needed to produce a specific amount of barium oxide, which is essential for preparing the desired concentration of hydroxide ions.

Molarity

Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is crucial for understanding how to prepare solutions with specific concentrations. In this question, knowing that we need a 0.10 M solution of OH- allows us to calculate the number of moles of hydroxide ions required, which directly relates to the amount of barium oxide produced.

Chemical Reactions and Products

Understanding the chemical reaction between barium and oxygen is essential for this problem. Barium reacts with oxygen to form barium oxide (BaO), and this reaction must be balanced to determine the stoichiometric coefficients. The formation of hydroxide ions from barium oxide in solution is also important, as it connects the mass of barium needed to the final concentration of hydroxide ions in the solution.

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Find the mass of barium metal (in grams) that must react with O2 to produce enough barium oxide to prepare 1.0 L of a 0.10 M solution of OH-.

Verified video answer for a similar problem:

Key Concepts

Stoichiometry

Molarity

Chemical Reactions and Products

Find the mass of barium metal (in grams) that must react with O₂ to produce enough barium oxide to prepare 1.0 L of a 0.10 M solution of OH^-.