Q1)What is the common ion in a solution that is saturated with the salts Na3PO4, Na2SO4, and AgCl?

Ag+, Na+, po4^3-, so4^2-, cl-

Q2What is the pH of a buffer made by adding 50.0mL of 0.200M HCl to 100.0mL of 0.400M NH3? pKa(NH4+)=9.26.

Do NOT use scientific notation!

Discuss the chemical reactions that occurred between glucose, fructose, xylose and sucrose and the 4 reagents(Benedict, Bial, Seilwanoff and Molisch) which have resulted in color changes. Describe how it occurs in full using the chemical makeup of the reagents.

Q1Ksp(CaF2)=3.9*10-11. What is the concentration of [F-] in equilibrium with solid CaF2?

0.00043m, 0.00027m, 0.00054m, 0.0021m

Q2The Ksp of silver acetate (Ag(H3C2O2)) is 2.0*10-3. What is the concentration of Ag+ in equilibrium with solid silver acetate in a solution that also contains 1.0M sodium acetate? Answer in molarity (M).

Do NOT use scientific notation!

Assuming standard conditions, answer the following questions. (Use the table of Standard Reduction Potentials for common Half-reactions from your text. If hydrogen is one of the reagents, assume acidic solution.)

1) Is Cr3+(aq) capable of oxidizing Fe2+(aq) to Fe3+(aq)?

2) Is Cr metal capable of reducing Fe2+(aq)?

3) Is Sn metal capable of reducing Fe3+(aq) to Fe2+(aq)?

4)Is H2(g) capable of reducing Ni2+(aq)?

5) Is Fe2+(aq) capable of reducing Cr3+(aq) to Cr metal?

6)Is VO2+(aq) capable of oxidizing Fe2+(aq)?

In Atomic Absorption Spectrophotometry (AAS) Lab, we ask to make a standard to determine the linear range of the Mg calibration.
"First make up a 100.0 ppm Mg solution. Then from the 100 ppm solution make up 25 mLs of 0.5, 1, 2, 5, 10 and 20 ppm Mg standards, then dilute it in a volumetric flask that contain 5 mL of 2% HNO3 solution and the rest with DW"
I have to use a micropipette (uL) to prepare the standard. How do I prepare the standards of ppm using (uL) micropipette??

Buffer preparation is a necessary part of working with any living cell culture. Buffers are most commonly prepared by starting with a weak acid, HA, or weak base, A-, and adding enough strong acid, H+, or strong base, OH-, to find the correct ratio of [HA]/[A-]. A pH = 7.3 buffer is needed in the lab. This buffer is made by first dissolving 52.25 g K2HPO4 in 400 mL of water. What is the pH of this salt solution? This solution of course will be too basic becuase we only have the base of the buffer present. What must the value of the ratio of [H2PO4-]/[HPO42-] be to create a buffer solution that is pH = 7.3? How many moles of HCl must be added to the 400 mL solution of HPO42-(aq) to prepare the pH = 7.3 buffer solution? How many mL of 1 M HCl must be added to the solution to create the pH = 7.3 buffer solution?

Consider the titration of a 22.0 −mL sample of 0.100 M HC2H3O2 with 0.130 M NaOH. Determine each quantity: (For acetic acid, HC2H3O2, Ka = 1.8 × 10^-5)

A) The initial pH.

B) The volume of added base required to reach the equivalence point.

C) The pH at 4.0 mL of added base.

D) The pH at the equivalence point.

E) The pH after adding 6.0 mL of base beyond the equivalence point.

Given a diprotic acid, H2A, with two ionization constants of Ka1 = 4.08× 10–4 and Ka2 = 2.89× 10–12, calculate the pH and molar concentrations of H2A, HA–, and A2– for each of the solutions below. (a) a 0.167 M solution of H2A (b) a 0.167 M solution of NaHA (c) a 0.167 M solution of Na2A

At 25 °C only 0.0650 mol of the generic salt AB2 is soluble in 1.00 L of water. What is the Ksp of the salt at 25 °C?

The decomposition of n2o5 is a first order reaction. N2o5 decomposes to yield no2 and o2.

At 48deg C the rate constant for the reaction is 1.2x10^-5s^-1. Calculate the partial pressure of no2 produced from 1.0L of 0.700M n2o5 solution at 48deg C over a period of 22 hours if the gas is collected in a 10.0L container. Show work please.

A certain weak acid, HA, with a Ka value of 5.61×10−6, is titrated with NaOH.

A solution is made by mixing 9.00 mmol (millimoles) of HA and 3.00 mmol of the strong base. This resulted in a pH of 4.95.

More strong base is added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 77.0 mL ?

Express the pH numerically to two decimal places.

Please help!! Please show steps if possible. THANK YOU!!

A chemical analysis of a surface water yields the following data:

Ion      Concentration (mg/L)

Ca2+ 90

Mg2+ 30

Na+ 72

K+ 6

Cl- 120

SO42- 225

HCO3- 165

pH 7.5

What concentration of Cl- (mg/L) would make the cations and anions balance?  

how much 5.80 M NaOH must be added to 460.0 mL of a buffer that is 0.0200 M acetic acid and 0.0250 M sodium acetate to raise the pH to 5.75

Arrange in order of increasing atomic size. (Use the appropriate <, =, or > symbol to separate substances in the list.)

(a) the Period 2 elements C, Ne, and O

(b) the Group 4A elements Ge, C, and Pb

A solution of household bleach contains 5.25% sodium hypochlorite, NaOCl, by mass. Assuming that the density of bleach is the same as water, calculate the volume of household bleach that should be diluted with water to make 500.0 mL of a pH = 10.18 solution.

= _________ mL