Determine the pH of each two-component solution. d. 0.088 M HClO 4 and 0.022 M KOH

Hello everyone today we are being asked to find the ph of the following two components solution. So we have 10 mL of 100.134 Mueller and A. O. H. And then we have 12.5 mL of 0.128 Mueller of HBR. So the first thing we wanna do is we want to find the number of moles of each component. So if you want to start with the first sodium hydroxide to find the number of moles of sodium hydroxide we can take our volume. We have 10 mL and the first they want to do is convert it to leaders with a conversion factor that one millimeter is equal to 10 to the negative third leaders. And then we want to multiply to get rid of the leaders. We can say that we have 0.134 moles per liter and moles per liter is the unit from hilarity. And so our units are going to cancel out to give us 0.00134 moles. And then for our Hbr or hydrogen bromide we have our moles of H B. R. We're gonna do the same procedure are at 12.5 moles 12.5 middle leaders. And we're going to convert that into liters by using the conversion factor that one mL equal to 10 to the negative third leaders. We're gonna multiply by the maturity which is 0.128 moles per one liter as before. Our units are going to cancel out and we're going to be left with 0.00160 moles. The next thing you wanna do is we want to set up an ice chart. So we're gonna set up our equation first, we're going to say that we have sodium hydroxide and we added HBR it's a two component system. And when they react they're gonna form sodium bromine And H 20. Or water. And so we're gonna set up our ice table I. C. E. Our initial concentration of sodium hydroxide is 0.134 moles for hbr 0.160 of course for N A B. R. And water. They're going to be both zero. We're going to subtract by the lowest number which is going to be our 0.00134 for both of our reactant here. But they were going to add it To our products plus 0.00134 moles. E. Is going to be the total. So it's going to be I plus C. In the case of sodium hydroxide, that's zero for hydrogen bromide. That's going to be 0.0 to +60. And then we're gonna do the same for our product side 600. and then the same for our water. So now we have to calculate the Milan city of HBR and use it to find the ph So we're going to say that our total volume of the solution is going to be that 10 mL plus the 12.5 mL to give us 22.5 middle leaders to find a concentration of our H B. R. We are simply going to take the number of moles that we end up with as our final. So 0.000-60 moles of HbR. And they were going to divide that by the total volume. So 0.225 mL. But of course you want this in leaders to find the polarity. So we're gonna use the conversion factor that one mL equal to 10 to the negative third Leaders. Our units of middle leaders are going to cancel out. We're gonna be left with 0.0116 Mohler hydrogen bromide is a strong acid. So we're going to see the concentration of that strong acid is going to equal the concentration of our hydro ni um ions or H plus ions. And so that makes it really simple when finding a ph the formula for phs negative log of the hydrogen concentration. And so we simply need to plug in the values that we have gotten so far. So we'll say negative log of 0. moller to give us a final ph of 1.936. I hope this helped. And until next time

Ch.16 - Acids and Bases

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Tro 4th Edition

Ch.16 - Acids and Bases

Problem 140d

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Chapter 16, Problem 140d

Determine the pH of each two-component solution. d. 0.088 M HClO₄ and 0.022 M KOH

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Identify the nature of the substances: HClO4 is a strong acid and KOH is a strong base.

Write the balanced chemical equation for the reaction: \( \text{HClO}_4 + \text{KOH} \rightarrow \text{KClO}_4 + \text{H}_2\text{O} \).

Calculate the moles of HClO4 and KOH using their concentrations and the volume of the solution (assuming 1 L for simplicity).

Determine the limiting reactant by comparing the moles of HClO4 and KOH.

Calculate the concentration of excess HClO4 or KOH after the reaction, and use it to find the pH or pOH, then convert to pH if necessary.

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Key Concepts

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

pH Scale

The pH scale measures the acidity or basicity of a solution, ranging from 0 to 14. A pH of 7 is neutral, below 7 indicates acidity, and above 7 indicates basicity. The scale is logarithmic, meaning each whole number change represents a tenfold change in hydrogen ion concentration. Understanding pH is crucial for analyzing the behavior of acids and bases in solution.

Strong Acids and Bases

Strong acids, like HClO4, completely dissociate in water, releasing all their hydrogen ions (H+), while strong bases, like KOH, fully dissociate to release hydroxide ions (OH-). This complete dissociation simplifies calculations of pH, as the concentration of the acid or base directly determines the concentration of H+ or OH- ions in the solution. Recognizing the strength of acids and bases is essential for accurate pH determination.

Neutralization Reaction

A neutralization reaction occurs when an acid reacts with a base to form water and a salt, typically resulting in a solution that is closer to neutral pH. In this case, the H+ ions from HClO4 will react with the OH- ions from KOH. The extent of this reaction influences the final pH of the solution, making it important to consider the stoichiometry of the reactants involved.

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Determine the pH of each two-component solution. a. 0.0550 M in HI and 0.00850 M in HF b. 0.112 M in NaCl and 0.0953 M in KF c. 0.132 M in NH₄Cl and 0.150 M HNO₃ d. 0.0887 M in sodium benzoate and 0.225 M in potassium bromide e. 0.0450 M in HCl and 0.0225 M in HNO₃

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Write net ionic equations for the reactions that take place when aqueous solutions of the following substances are mixed: a. sodium cyanide and nitric acid b. ammonium chloride and sodium hydroxide c. sodium cyanide and ammonium bromide d. potassium hydrogen sulfate and lithium acetate e. sodium hypochlorite and ammonia

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Determine the pH of each two-component solution. d. 0.088 M HClO4 and 0.022 M KOH

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Key Concepts

pH Scale

Strong Acids and Bases

Neutralization Reaction

Determine the pH of each two-component solution. d. 0.088 M HClO₄ and 0.022 M KOH