(d) If 42.7 mL of 0.208 M HCl solution is needed to neutralize a solution of Ca(OH) 2 , how many grams of Ca(OH) 2 must be in the solution?

Hello everyone. So in this video we need to go ahead and calculate the mass of sodium carbonate required to completely neutralize the acid. So they give us the neutralization equation here. So go ahead and use it for our multiple ratios. Alright, so first we're given that we have 600 ml of this concentration of hcl. So that's how we'll start off our dimensional analysis. So again we're starting off with 600 ml of hcl. We want to convert our millions and are leaders. So we can go ahead and utilize our polarity. So convert our middle leaders and to leaders. And then we can go ahead and use our maturity as our second conversion factor. So let's go ahead and recall that capital M. So polarity is equal to most her leader. So then we have 0. moles of hcl for every one liter of solution. So so far we can see that our male leaders will cancel. Leaders will cancel. All right, So now we're stuck with here the moles of Hcl again, we need to go ahead and look for the moles of our N. A. To C. 03 are sodium carbonate. So now we can go ahead and do a multi mole ratio here. So you see from our reaction that's given to us in the problem that for every two moles of hcl We'll need one mole of sodium carbonate. Now you can see that the moles of Hcl will cancel. Now it says we need to calculate the mass and that's usually in the units of grams. How we can get that is by using the molar mass of sodium carbonate, which you can either find online calculator itself or it can be given to you by professor. So here what I have is that for every one mole of our sodium carbonates That equals to 105. g of sodium carbonate. Alright, now we can see that the moles of sodium carbonate. Well, council so putting this into my calculator, I'll get the numerical value of 9. and units being grams of sodium carbonates. So that's how much it takes to completely neutralize our hydrochloric acid here.

Ch.4 - Reactions in Aqueous Solution

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Brown 14th Edition

Ch.4 - Reactions in Aqueous Solution

Problem 82d

Chapter 4, Problem 82d

(d) If 42.7 mL of 0.208 M HCl solution is needed to neutralize a solution of Ca(OH)₂, how many grams of Ca(OH)₂ must be in the solution?

Verified step by step guidance

Start by writing the balanced chemical equation for the neutralization reaction between HCl and Ca(OH)2:

{Ca (OH) 2}_{(aq)} + 2 {HCl}_{(aq)} \to {CaCl (aq)}_{2} + 2 {H (O H)}_{(l)}

Calculate the moles of HCl used in the reaction. Use the formula:

moles = volume \times molarity

. Convert the volume from mL to L by dividing by 1000.

Using the stoichiometry from the balanced equation, determine the moles of Ca(OH)2 that reacted. According to the equation, 2 moles of HCl react with 1 mole of Ca(OH)2. Therefore, divide the moles of HCl by 2 to find the moles of Ca(OH)2.

Calculate the mass of Ca(OH)2 using its molar mass. The molar mass of Ca(OH)2 is the sum of the atomic masses of Ca, O, and H:

molar mass = 40.08 + 2 \times (16.00 + 1.01)

. Multiply the moles of Ca(OH)2 by its molar mass to find the mass in grams.

Ensure all units are consistent and check your calculations for accuracy. This will give you the mass of Ca(OH)2 required to neutralize the given amount of HCl.

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Key Concepts

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

Neutralization Reaction

A neutralization reaction occurs when an acid reacts with a base to produce water and a salt. In this case, hydrochloric acid (HCl) reacts with calcium hydroxide (Ca(OH)2). The balanced chemical equation for this reaction is 2 HCl + Ca(OH)2 → CaCl2 + 2 H2O, indicating that two moles of HCl are required to neutralize one mole of Ca(OH)2.

Molarity and Volume Relationship

Molarity (M) is defined as the number of moles of solute per liter of solution. To find the number of moles of HCl used in the reaction, you can use the formula: moles = molarity × volume (in liters). In this problem, the volume of HCl is given in milliliters, so it must be converted to liters before calculating the moles.

Stoichiometry

Stoichiometry involves using the coefficients from a balanced chemical equation to relate the amounts of reactants and products. In this case, knowing the moles of HCl allows you to determine the moles of Ca(OH)2 that reacted, and subsequently, you can convert moles of Ca(OH)2 to grams using its molar mass. This is essential for solving the problem accurately.

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(a) How many milliliters of 0.120 M HCl are needed to completely neutralize 50.0 mL of 0.101 M Ba(OH)₂ solution?

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(b) How many milliliters of 0.125 M H₂SO₄ are needed to neutralize 0.200 g of NaOH?

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(c) If 55.8 mL of a BaCl₂ solution is needed to precipitate all the sulfate ion in a 752-mg sample of Na₂SO₄, what is the molarity of the BaCl₂ solution?

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Textbook Question

The distinctive odor of vinegar is due to acetic acid, CH3COOH, which reacts with sodium hydroxide according to: CH3COOH1aq2 + NaOH1aq2¡ H2O1l2 + NaCH3COO1aq2 If 3.45 mL of vinegar needs 42.5 mL of 0.115 M NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in a 1.00-qt sample of this vinegar?

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Textbook Question

A 4.36-g sample of an unknown alkali metal hydroxide is dissolved in 100.0 mL of water. An acid–base indicator is added, and the resulting solution is titrated with 2.50 M HCl(aq) solution. The indicator changes color, signaling that the equivalence point has been reached, after 17.0 mL of the hydrochloric acid solution has been added. (a) What is the molar mass of the metal hydroxide?

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(d) If 42.7 mL of 0.208 M HCl solution is needed to neutralize a solution of Ca(OH)2, how many grams of Ca(OH)2 must be in the solution?

Verified video answer for a similar problem:

Key Concepts

Neutralization Reaction

Molarity and Volume Relationship

Stoichiometry

(d) If 42.7 mL of 0.208 M HCl solution is needed to neutralize a solution of Ca(OH)₂, how many grams of Ca(OH)₂ must be in the solution?