In a titration of 47.76 mL of 0.3886 M nitrous acid with 0.3886 M aqueous sodium hydroxide, what is the pH of the solution when 47.76 mL of the base have been added?

A rigid container whose volume can be varied with the use of a piston contains 2.53 mol H₂ gas at STP.

(a) What is the volume of the gas?
_____L

(b) The container is cooled to 209 K. The piston is held fixed so the volume does not change. What is the new pressure inside the container?
____atm

(c) The temperature of the container is held at 209 K and 1.55 mol He gas is added to the container. The pressure inside the container is held constant, but the piston is released so the volume of the container can vary. What is the final volume of the container?
_____ L

(d) What are the partial pressures of H₂ and He in the container in part (c)?

(e) The piston on the container in part (c) is set to maintain a constant pressure of 1 atm. The container is then heated from 209 K to 380 K.What is the minimum amount of heat that must be added to the container for it to reach 380 K?
______ J

Calculate ΔG° for the following reaction as written

Ni²⁺ (aq) + Sn (s) → Ni (s) + Sn²⁺ (aq)

given the following reduction half-reactions and standard reduction potentials.

Sn²⁺ (aq) + 2 e^- → Sn (s)      E° = -0.15V

Ni²⁺ (aq) + 2 e^- → Ni (s)      E° = -0.25V

Calculate the density of oxygen, O 2 , under each of the following conditions: STP 1.00 atm and 35.0 ∘ C Express your answers numerically in grams per liter. Enter the density at STP first and separate your answers by a comma.

What is the molar solubility of AgCl in 0.1 M HCl? How many grams of silver chloride will dissolve in 500 mL of 0.1 M HCl? show all calculations

identify and then write the balance chemical equation for each salt below that will yield a basic solution in water

i. NH4Br ii. NaCN iii. BaF2 iv. NaNO3

A total volume of 33.15-mL of 0.1053-M NaOH is needed to titrate 24.5-mL of benzoic acid. (Benzoic acid is a monoprotic acid with a pKa = 4.20). Determine the pH when the following volumes of the 0.1053 M NaOH have been added

a) 30.00 mL (before the equivalence point)?

b) 33.15 mL (at the equivalence point)

c) 36.00 mL (after the equivalence point)

NH3 is a weak base (Kb = 1.8 × 10–5) and so the salt NH4Cl acts as a weak acid. What is the pH of a solution that is 0.038 M in NH4Cl at 25 °C?

Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.150 M HClO(aq) with 0.150 M KOH(aq). The ionization constant for HClO can be found here.

(a) before addition of any KOH (b) after addition of 25.0 mL of KOH (c) after addition of 35.0 mL of KOH (d) after addition of 50.0 mL of KOH (e) after addition of 60.0 mL of KOH

a. Use standard cell potentials to show what reaction would occur if you placed a strip of Cr in a solution of equal concentrations of NiCl2 and Al(NO3)3.

b. Zinc is plated onto iron to protect the iron from corrosion in a process called galvanization. How long would it take to plate 100g of zinc onto “sheet metal” in a ZnCl2 bath running at a current of 7.5A?

Promise to rate! Much appreciated, thank you!

You are shoveling bituminous Pennsylvania coal (with an energy content of 13,870 Btu/lb) from a coal box into a furnace. On average, with each lift and throw, you raise a 1.8 kg shovel containing 4.7 kg of coal by a height of 0.85 m. Assume your body is working with an efficiency of 15.9%. How many thousands of times more chemical energy is in the coal you move than is in the sugars and fats your body is burning to move it?

Benzene and ethylbenze are to be separated in a single-stage flash vessel. The resulting liquid stream must have a composition of x₁= 0.35 and the resulting vapor stream must have a composition of y₁= 0.75. You may assume Raoult's law applies.

a) Determine what T and P must be in the vessel in order to carry out this separation, show all work and equations used.

b) What additional information is needed to compute the relative amounts of liquid and vapor leaving the vessel?

Calculate the pH of each of the solutions and the change in pH to 0.01 pH units caused by adding 10.0 mL of 2.05-M HCl to 570. mL of each of the following solutions.

a) water  

before mixing = 7

After mixing = 1.45

b) 0.135 M C₂H₃O₂^1-

^{Before mixing = 8.95}

^{After mixing = ?}

c) 0.135 M HC₂H₃O₂

_{Before mixing = ?}

_{After mixing = ?}

d) a buffer solution that is 0.135 M in each C₂H₃O₂^1- and HC₂H₃O₂

_{Before mixing = ?}

_{After mixing = ?}

I've tried this so many times and I don't understand it. Is there a formula or a set of formulas for this ?? Can someone please just spell it out for me step by step and why. Please and thank you!

If a solution containing 39.544 g of mercury(II) perchlorate is allowed to react completely with a solution containing 13.180 g of sodium dichromate, how many grams of solid precipitate will be formed?

How many grams of the reactant in excess will remain after the reaction?