### Solubility of CuBr in Different Aqueous Solutions**Question:** In which of the following aqueous solutions would you expect CuBr to have the highest solubility?**Options:**- **A.** CuBr will have the same solubility in all solutions.- **B.** 0.040 M CuNO₃- **C.** 0.0100 M KBr- **D.** 0.030 M NaBr- **E.** 0.020 M LiBr**Explanation:**To understand where CuBr (Copper(I) bromide) would have the highest solubility, we need to consider the common ion effect and the solubility product constant (Ksp). The addition of a common ion (in this case, Br⁻) can decrease the solubility of CuBr as it shifts the equilibrium to the left according to Le Chatelier's Principle. Therefore, the solution with the highest concentration of the common ion Br⁻ will have the lowest solubility for CuBr, and the solution without any common ions will have the highest solubility for CuBr.In this context:- **Option A** is incorrect because solubility won't be the same in all solutions due to the common ion effect.- **Option B** involves CuNO₃, which does not provide Br⁻ ions. Therefore, it won’t contribute to the common ion effect, resulting in higher solubility of CuBr.- **Options C, D, and E** each contain Br⁻ ions from KBr, NaBr, and LiBr, respectively, which will decrease the solubility of CuBr due to the common ion effect.Hence, among the given options, **Option B (0.040 M CuNO₃)** is where CuBr is expected to have the highest solubility.

Given that : We have to determine, in which of the following aqueous solutions will CuBr have the…

In which of the following aqueous solutions would you expect CuBr to have the highest solubility? Select one: O A. CuBr will have the same solubility in all solutions. O B. 0.040 M CUNO3 O C. 0.0100 M KBr O D. 0.030 M NaBr O E. 0.020 M LİBR

In which of the following aqueous solutions would you expect CuBr to have the highest solubility? Select one: O A. CuBr will have the same solubility in all solutions. O B. 0.040 M CUNO3 O C. 0.0100 M KBr O D. 0.030 M NaBr O E. 0.020 M LİBR

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

At 25 °C and 765 Torr, carbon dioxide has a solubility of 0.0342 M in water. What is its solubility at 25 °C and 2010 Torr?
The Ksp for silver iodate, AglO3, is 3.2 × 10⁹. How many grams of silver would be dissolved in 10 liters of a saturated solution of silver iodate? a. 0.51 g b. 0.22 g c. 0.19 g d. 1.8 g e. 2.2 g
The solubility of silver bromate, AgBrO3, in water is 7.2 x 10- g/L. Calculate Ksp.
96. Water pollution. The use of iodine crystals is a popular way of making small quantities of water safe to drink. Crystals placed in a 1-ounce bottle of water will dissolve until the solution is saturated. After saturation, half of the solution is poured into a quart container of water, and after about an hour, the water is usually safe to drink. The half-empty 1-ounce bottle is then refilled, to be used again in the same way. Suppose that the concentration of iodine in the 1-ounce bottle t minutes after the crystals are introduced can be approximated by C(t) = 250(1-e) t≥ 0 where C(t) is the concentration of iodine in micrograms per milliliter. (A) What is the rate of change of the concentration after 1 minute? After 4 minutes? (B) Graph C for 0 ≤t ≤ 5.
PCI5(g) → PCI3(g) + Cl2(g) has K, = 1.84 at a given temperature. What is the value of K, for the reaction PCI3(g) + Cl2(g)PCI5(g) at the same temperature? %3D 1.84
What is the molar solubility of MgF2 in a 0.40 M Mg(NO3)2 solution? For MGF2, Ksp = 9 x 108. %3D a. 3.2 x 104 M O b. 2.4 x 10 4 M c. 1.8 x 104 M O d. none of these Oe. 5.6 x 10-8 M
In a system of NaCl and water is at dynamic equilibrium, when more table salt is added it will appear that the added salt does not dissolve in the solution. O True O False MacBook 80 000 000 DII DD F2 F3 F4 F5 F6 F7 F8 F9 F10 $4 & *
8. Solubility of CrF3 in water is 0.102 g/L at 25 oC. What is the molar concentration of F- ionin the solution at the same temperature?A. 3.30 x 10-3 B. 3.97 x 10-11 C. 1.10 x 10-2 D. 2.80 x 10-3 E. 3.10 x 10-4
16. Concentrated glacial acetic acid is 99.7% H3CCO2H by mass and has a density of 1.05 g/mL. What is the molar concentration of concentrated glacial acetic acid? Group of answer choices A. 1750 M B. 17.5 M C. 1.75 M
Tiny samples of aqueous solutions are sketched below, as if under a microscope so powerful that individual molecules could be seen. (The water molecules are not shown.) The two substances in each sample can interconvert. That is, each kind of molecule can turn into the other. The equilibrium constant K for each interconversion equilibrium is shown below the sketch. Decide whether each solution is at equilibrium. K= K=1 At equilibrium? At equilibrium? O yes O no O yes O no 000 000 000 - =+ K=- K= At equilibrium? At equilibrium? O yes O no O yes no Explanation Check Accessibility Privacy O 2021 McGraw-Hill Education. All Rights Reserved. Terms of Use
10. Which factor will not increase the concentration of NH3 (ammonia)? N2(g) + H2(g) 2 NH3(g) + heat A. Increasing the concentration of H2. B. Increasing the concentration of N2. C. Decreasing the pressure. D. Decreasing the temperature.
17. A certain drug binds to a protein with Kd = 850.0 nM. What initial concentration of the drug would you need to add to a 50.0 µM solution of the protein so that 95.0% of the protein molecules are drug-bound at equilibrium? А. 1.62 µM В. 16.2 иМ С. 47.5 µM D. 52.6 µM Е. 63.7 иМ