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A 1.0 - $L$ saturated silver carbonate solution at $5^{\circ} \mathrm{C}$ is treated with enough hydrochloric acid to decompose the compound. The carbon dioxide generated is collected in a $19-\mathrm{mL}$ vial and exerts a pressure of $114 \mathrm{mm} \mathrm{Hg}$ at $25^{\circ} \mathrm{C}$. What is the $K_{\mathrm{sp}}$ of $\mathrm{Ag}_{2} \mathrm{CO}_{3}$at $5^{\circ} \mathrm{C} ?$

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$$6 \cdot 2 \times 10^{-12}$$

Chemistry 102

Chapter 16

Acid-Base Equilibria and Solubility Equilibria

Acid-Base Equilibria

Aqueous Equilibria

University of Central Florida

Rice University

University of Kentucky

University of Toronto

Lectures

00:41

In chemistry, an ion is an atom or molecule that has a non-zero net electric charge. The name was coined by John Dalton for ions in 1808, and later expanded to include molecules in 1834.

24:14

In chemistry, a buffer is a solution that resists changes in pH. Buffers are used to maintain a stable pH in a solution. Buffers are solutions of a weak acid and its conjugate base or a weak base and its conjugate acid, usually in the form of a salt of the conjugate base or acid. Buffers have the property that a small change in the amount of strong acid or strong base added to them results in a much larger change in pH. The resistance of a buffer solution to pH change is due to the fact that the process of adding acid or base to the solution is slow compared to the rate at which the pH changes. In addition to this buffering action, the inclusion of the conjugate base or acid also slows the process of pH change by the mechanism of the Henderson–Hasselbalch equation. Buffers are most commonly found in aqueous solutions.

03:38

If wet silver carbonate is…

01:05

A saturated solution of s…

01:51

03:05

A $1.00-\mathrm{L}$ soluti…

02:50

$K_{\mathrm{sp}}$ for magn…

03:45

The dissociation of calciu…

01:19

Carbon dioxide can be made…

04:26

For the decomposition of s…

Hello. So today we're going to be looking at a situation. We have one leader of a known concentration off silver carbonate and what we've done is we've added hydrochloric acid. And basically, what's happened is this I on Plus these protons reacted and that created it carbon dioxide in water. And so we've taken the carbon dioxide that was produced and we found and we put it into a a vial that 19 milliliters and volume. We found that at 25 degrees Celsius it gave off a pressure of 114 milliliters. Leaders of mercury. So first start off. How about we find out how much carbon, how many moles of carbon dioxide we have So we know the volume, the pressure on the temperature. So why don't we just use that ideal gas law pressure times Volume equals the moles. Times toe are in temperature. So the volume we have to have in leaders Celeste ified by 1000 we'll see we have zero point 019 leaders 1,000,000 meters of mercury. One atmosphere is equal to 760 million millimeters of mercury. So let's divide. And when we divide, we will see that we have zero 0.12 atmospheres of pressure and then we need to switch it the Celsius to Calvin. So just add 273. So we have 200 and 98 Calvin. So how about now we plug in so our pressure is 0.12 I mean, 15 atmospheres. Time 0.19 Leaders is equal to moles times the rate cost instant which is 0.8 206 litters atmospheres for Calvin and mul and then the temperature is 298 Calvin So let's solve firm ALS and we see well as we solve this that we have 0.0 117 moles of carbon dioxide. So now we know how many moles of carbon dioxide we have and from our reaction above we see that one mole of carbon dioxide corresponds to one mole off carbonate. So that means that we have 0.117 moles of carbonate. So now how about we write the so the ability equilibrium for silver carbonate. So we see that when if when we're dissolving the silver carbonate. We'll see that we'll get two of the Mueller Celje bility for silver's because their two moles of silver per mole of silver carbonate and one mall and one as of but carbon e ions. So the Casspi would be concentration of the silver squared and the concentrations of carbonate so that great constant Kirsty would be to us squared times s which would be for as cute so us eso the concentration of the carbonate would be us. And so we have 0.117 moles and that's in one leader. So that would be the molar ity. So we see that the Casspi is equal to four times zero, 0.0 117 cubed. So we take our answer, Cubitt and then times it by four we will see that are Casspi is equal to 6.3 times 10 to the negative 12

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