At a temperature other than 25^oC, Cd(OH)₂ solubility is 5.5 x 10^-4 . Calculate it's Ksp at this temperature.

[ACCORDING TO MY TEXT, Ksp of Cd(OH)₂ = 2.5 x 10¹⁴ @ 25 C]

A.1.7 x 10^-10

B.6.7 x 10^-10

C.2.5 x 10^-14

1.   An electrode of solid chromium is immersed in a 1M solution of Cr³⁺; In a second beaker, a tin electrode is immersed in a 1 M solution of Sn²⁺. The two electrodes are connected by a wire through a voltmeter, and the two beakers are connected via a salt bridge. The entire system is maintained at a T = 298K. When the connection is made between the two cells, what is the E^o for the cell, in volts, if the reduction potential for Cr(III) to Cr(0) is -0.74 V and the reduction potential for Sn(II) to Sn(0) is -0.14V? (a) –0.78V (b) 0.78V (c) –0.60V (d) 0.60V (e) none of these

2.   Using the data in the table provided, calculate the approximate standard state Gibbs free energy change at 298 K for the reaction Al₂O_3(s) + 3H_2(g) => 2Al_(s) + 3H₂O_(g)

   (a) 236 (b) 886 (c) –344 (d) –1021 (e) none of these

3. The K_sp for lead (II) fluoride in water is 3.6 x 10^-8. What is its solubility in g/L? (a) 3.3 x 10^-3 (b) 1.3 x 10^-4 (c) 0.051 (d) 2.1 (e) none of these

4. The lower the vapor pressure of a liquid, the (a) higher the boiling point (b) the lower the boiling point (c) the higher the melting point (d) the lower the melting point (e) none of these relationships are true.

5. Elemental phosphorous, which exists as P₄ molecules, has the following solubility properties: Water – insoluble; CCl₄ – soluble. What may be ascertained about the type of intermolecular forces which are operative when P₄ forms solutions? (a) they are ion-dipole in nature (b) they are dipole-dipole in nature (c) they are London force in nature (d) they are ionic in nature (e) they are covalent in nature

6. What is the order of the reaction in NO? (a) -1 (b) 0 (c) 1 (d) 2 (e) none of these

7. What is the order of the reaction in H₂? (a) -1 (b) 0 (c) 1 (d) 2 (e) none of these

Consider the reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kc=102 at 500 K A reaction mixture initially contains 0.135 M CO and 0.135 M H2O. What is the equilibrium concentration of [CO], [H2O], [CO2], and [H2]

compare the values of the enthalpy of neutralization for the three acids( H3CCOH, Na2S2O3, HCl). explain any similarities and/or differences

Find the pH of a 0.14M CH3COOH solution. Ka= 1.8x 10^-5

Fill in the blanks using (fatty acids, glycerol, sphingolipids, steriods, glycolipids, glycerophospholipid, triacylglycerols.)

Compounds that contain a fused ring system are called __________. These have three 6-membered rings and one 5-membered ring. Some of these compounds are found in biological membranes. _________ are the building blocks for many lipids, and they generally contain an even number of carbon atoms and an unbranched hydrocarbon chain. ________ are formed when a carbohydrate is glycosidically linked to a hydroxyl group of a lipid. Examples include gangliosides and cerebrosides. These are found in biological membranes. ________ are the storage form of lipids, accumulating in adipose tissue, and they can be used as metabolic fuel. These compounds have a polar part, made of three ester groups, and a nonpolar fatty acid tail. They behave as all nonpolar. ________ are made up of a long-chain amino alcohol joined, either by a glycosidic linkage and a phosphodiester linkage, to a fatty acid. These do not contain ______. They are abundant in the nervous system. When glycerol is esterfied to two fatty acids and a phosphoric acid molecule a _____ is formed. These are found in biological membranes.

Hydrogen and chlorine gas are placed in a 10.0 L container and allowed to react. The initial density of the mixture is 5.01 x10-3 gm/ml. The vessel is at 300K and the initial pressure is 6.52 atm. After the reaction is complete , the pressure is 6.52 atm. The gas is bubbled into 1.00 liter of deionized water. In another part of the universe, a grey haired chemistry instructor prepares an acetic acid/ acetate buffer. The buffer was prepared by adding acetic acid and sodium acetate to 2.50 L of deionized water. Now, as universes collide, our hero adds 107 ml of the HCl solution to 405 ml of the buffer. The pH is measured and is 4.35 after the HCl addition. A drop of phenolphthalein is added and the solution is titrated to equivalence with 657 ml of 0.920 M NaOH. Calculate the original molarities of the weak acid and conjugate base in the 2.50 L solution?

To prepare a buffer properly, it is essential to understand how a buffer is described. Here are four buffers used:

1. A solution that is 0.1 M HC2H3O2 and 0.10 M NaC2H3O2

2. One part 0.10 M NH3 mixed with one part 0.10 M NH4Cl

3. A solution that is 0.10 M NH3 and 0.20 M NH4Cl

4. Three parts 0.10 M NH3 mixed with one part 0.10 M HCl

For the first and third buffers, the concentrations of each component are explicit. What are the identities of and concentrations of the buffer components in the second and third buffers? (Keep in mind when mixed, the original solutions dilute each other)

Buffer 2:

Buffer 4:

In paper chromtography, what is the nature of the attractions between the stationary phase (cellulose) and the moving phase (hydrochloric acid/water/acetone) and the species ( Zn2+, Co2+, Cu2+, Cd2+ , Fe3+, and Ni2+ in two unknown solutions)  being separated, in particular what affects the Rf values and how?

Note: Filter paper (Whatman #1) serves as the stationary phase, and the mobile phase consists of a mixture of acetone and 6 M hydrochloric acid. A single spot of the mixture to be analyzed is applied near one edge of a sheet of filter paper. A spot of solution containing each of the cations that might be in the unknown mixture is also placed near the edge of the same sheet for comparison. The treated strip is then placed in a covered jar or beaker (which acts as a developing chamber) containing a shallow layer of the solvent mixture (see Figure 3). Since filter paper is very permeable to the solvent, the solvent begins to rise up the strip by capillary action. The various spots on the developed chromatogram will be highlighted by treatment with several chemical reagents to enhance their color. The reagents to be used are ammonia, dimethylglyoxime (DMG), and 8–hydroxyquinoline (oxine)

Derive an equilibrium relationship (y = f (x)) with relative volatility in the ideal solution

Determine the number of translational, rotational and vibrational degrees of freedom of HCl, CO2, H2O, NH3, and CH4.

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) sodium hydrogen sulfite and potassium cyanide

E) sodium hypochlorite and ammonia

A solution is 0.020 M in each Ca²⁺ and Cd²⁺. Adjusting the pH of the solution to which of the following values would achieve the best separation by precipitation of the hydroxides? solubility product constants

Best pH =  ---Select--- 13.0 12.5 12.0 11.5 11.0 10.5 10.0 9.5 9.0 8.5 8.0

What would be the resulting concentrations of the ions if the solution were adjusted to this pH?

[Ca²⁺] =  M

[Cd²⁺] =

M

Based on your copper solid used in RXN 1, how many grams of copper product should have been formed? Based on the copper solid in RXN 1, how many grams of the copper Hydroxide should have been formed in RXN 2? Based on the mass of copper used in RXN 1, how many grams of the zinc metal should have been used in RXN 5?

My mass of copper in RXN 1: .3595 grams

RXN1 : 4HN0₃ (aq) + Cu(s)-> Cu(NO₃)₂(aq) + 2H₂O (l) + 2NO₂ (g)

RXN 2: Cu(NO₃)₂(aq) + 2NaOH(aq) -> Cu(OH)₂(s) + 2NaNO_3(aq)

RXN 5: CuSO_4(aq)+ ZN(s) -> Cu (s) + Zn SO₄ (aq)       ( Mass of zinc in RXN 5: 3.00g)

Please show all work. I am confused on how to do this.