Calculate the pH of the solution at each step after the addition of i) 0.00mL ii) 2.30 mL, iii) 10.0 and iv) 16.0 mL of 0.50 M HCL to 100.0 mL of 0.10 M NH₃ solution.

The ΔG°\' of the reaction is -7.050 kJ ·mol–1. Calculate the equilibrium constant for the reaction. (Assume a temperature of 25° C.What is ΔG at body temperature (37.0° C) if the concentration of A is 1.8 M and the concentration of B is 0.75 M?

Identify the following species as electrolytes or nonelectrolytes:

CH₃OH

NH₄Cl

Ca(OH)₂

C₆H₆

RbClO₄

A titration involves adding a reactant of known quantity to a solution of an another reactant while monitoring the equilibrium concentrations. This allows one to determine the concentration of the second reactant. The equation for the reaction of a generic weak acid HA with a strong base is

HA(aq)+OH?(aq)?A?(aq)+H3O+(aq)

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

Part A:

A solution is made by titrating 9.00mmol (millimoles) of HA and 3.00mmol of the strong base. What is the resulting pH?

Part B:

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 45.0mL ?

How can you determine which compound is a stronger acid/base if neither compound is a strong acid or a strong base? Chapter 16, question 45 c. in chemistry a molecular approach textbook

Out of the choices provided, which is the best recrystallizing solvent for resorcinol and why?

a. Water

b. Petroleum ether

c. Ethanol

The equilibrium constant (Kp) for the following reaction is 4.40 at 2000.K.

H_2(g) + CO_2(g) <=> H₂O_(g) + CO_(g)

a) Calculate Delta G^o for the reaction. ____________ KJ/mol

b) Calculate Delta G for the reaction when the partial pressures are P_H2 = 0.28 atm, P_CO2 = 0.81 atm, P_H2O = 0.63 atm, and P_CO = 1.17 atm. ______________ KJ/mol

An equilibrium mixture contains 0.20 moles of hydrogen gas, 0.80 moles of carbon dioxide, 0.10 moles of carbon monoxide, and 0.40 moles of water vapor in a 1.00-liter container. How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.20 moles? The equation for the reaction is:

CO_(g)+H₂O_(g) <=> CO_{2 (g)}+H_{2 (g)}

Determine the EMF of this equation 2Fe + 6HCl ----> 2FeCl3 + 3H2

and what is that Reduction and Oxidation.

Hydrogen is mixed with a stoichiometric amount of oxygen in a 1 L volume at 100 kPa at 300 K. All of the hydrogen is burned at constant but heat leaves the system such that the final temperature is still 300 K. What is the amount of heat released and what is the final pressure in the container?

The density of water at room temperature is less than the assumed 1.0 g/mL used in the calculations for determining the enthalpy of neutralization. How will this small (but real) assumption affect the reported enthalpy of neutralization for the strong acid-weak base reaction? Explain.

How much heat (in kj) is needed to convert 866g of ice at -15*C to steam at 146*C? (Note: The specific heat of ice is 2.03J/g*C and the specific heat of steam is 1.99J/g*C. Delta fus for H20 is 6.01 kj/mol and Hvap is 40.79kj/mol)

Calculate the pH during the titration of 25.00 mL of 0.1000 M LiOH(aq) with 0.1000 M HI(aq) after 24.2 mL of the acid have been added. Explain.

The Ka’s for H₂SeO₂ are K1 = 2.7 x 10^-3 K2 = 2.5 x 10^-7 Calculate the pH of a solution formed when 30.0 mL of 0.25 M KSeO3 is mixed with a) 1.5 mL of 0.20 M KOH b) 20.0 mL of 0.25 M HCl c) 25.0 mL of 0.20 M K₂SeO₃

I know how to calculate pH's however, I do not know when to use K1 vs K2, can you explain please?