Calculate the [H⁺], [OH^-], pH, pOH for the resulting solution if 20.00 mL sample of 0.2650 M NaOH was titrated with 21.33 mL of 0.1175 M H₂SO_4.

19. A. Solid calcium nitrate is slowly added to 175 mL of a 0.0676 M potassium carbonate solution. The concentration of calcium ion required to just initiate precipitation is _____ M.

B. Solid zinc acetate is slowly added to 125 mL of a 0.0515 M potassium cyanide solution. The concentration of zinc ion required to just initiate precipitation is _____ M.

C. Solid sodium hydroxide is slowly added to 150 mL of a 0.0435 M copper(II) acetate solution. The concentration of hydroxide ion required to just initiate precipitation is _____ M.

Caproic acid is composed of C, H, and O atoms. The combustion of a 0.225g sample yields 0.512g of CO2 and 0.209g of H2O. What is the empirical formula for the compound?

A 1.00 L flask is filled with 1.45 g of argon at 25 ∘C. A sample of ethane vapor is added to the same flask until the total pressure is 1.450 atm .

What is the partial pressure of ethane, Pethane, in the flask? Express your answer to three significant figures and include the appropriate units.

Determine the vapor pressure of a solution at 55°C that contains 34.2 g NaCl in 375 mL of water. The vapor pressure of pure water at 55°C is 118.1 torr. The van't Hoff factor for NaCl is 1.9

interrelationship between global warming, acid rain, ozone layer depletion, and photochemical smog?

12.       What is responsible for capillary action, a property of liquids?

a)         surface tension

b)         cohesive forces

c)         adhesive forces

d)         viscosity

e)         two of these

32. Which of the following correctly states the relationship between temperature and the solubility of a substance in water?

a) The solubility of a substance in water increases as the temperature rises, especially for gases. b) The solubility of a substance in water decreases as the temperature rises, especially for ionic solids. c) The solubility of a substance in water with temperature cannot be accurately predicted, especially for ionic solids. d) The solubility of a substance in water decreases as the temperature lowers, especially for gases. e) Both A and D are correct.

Find the pH during titration of 20.00ml of 0.1000 M triethylamine, (CH3CH2)3N (Kb=5.210^-4), with 0.1000M HCL solution after the following additions of titrants a) 10.00mL b) 20.70 mL c) 27.00 mL

calculate the pH for a strong acid + strong base titration in which 5.00 mL of the M(OH)₂ was transferred via pipet to a beaker and HCl was added from the buret.

Concentration of base is 0.0721 M

Concentration of acid is 0.0524 M

Please show work.

Calculate the pH:

a) before any HCl is added

b) after the addition of 4.00 mL HCl

c) after the addition of 9.00 mL HCl

d) 4.00 mL beyond the equivalence point

Problem 5: Find the differential and total cross sections in the first Born approximation for elastic scattering of a particle of mass m, which is initially traveling along the z-axis, from a nonspherical, double-delta potential V (~ r) = V0δ(~ r − aˆ k)+V0δ(~ r+aˆ k), where ˆ k is the unit vector along the z-axis.

A combustion analysis of a 0.44g sample of an unknown compound yields 0.88 g CO2 and 0.36 g H2O. If the sample a molar mass of 132 g/mol, what is the molecular formula of the sample?

7. You are given 2.263 g of a mixture of KClO3 and KCl. When heated, the KClO3 decomposes to KCl and O2, 2 KClO3 (s) → 2 KCl (s) + 3 O2 (g), and 632 mL of O2 is collected over water at 20 °C. The total pressure of the gases in the collection flask is 736 torr. What is the weight percentage of KClO3 in the sample? The formula weight of KClO3 is 122.55 g/mol. The vapor pressure of water at 20 °C is 17.5 torr.

Imagine that you are in chemistry lab and need to make 1.00 L of a solution with a pH of 2.50. You have in front of you

100 mL of 6.00×10−2 M HCl,

100 mL of 5.00×10−2 M NaOH,

and plenty of distilled water.

You start to add HCl to a beaker of water when someone asks you a question. When you return to your dilution, you accidentally grab the wrong cylinder and add some NaOH. Once you realize your error, you assess the situation. You have 82.0 mL of HCland 87.0 mL of NaOH left in their original containers.

Assuming the final solution will be diluted to 1.00 L , how much more HCl should you add to achieve the desired pH?