You require 60 mL of a 5% solution. You have a stock solution available to you in 8% strength. How much of your stock solution is needed to make this new solution?

A 5% solution is what in mg/mL?  

Assuming complete dissociation and ideal solution behavior, calculate the freezing point depression of a solution of 0.824 g of NaCl (58.44 g/mol) in 133 g of water (Kf = 1.86 ∘C·kg).

Ammonium chloride (NH₄Cl) is a salt that dissolves completely in water. The ammonium ion (NH₄⁺) acts as a weak acid with a Ka of 5.1 × 10⁻10. If a 0.050 M solution of NH₄Cl is prepared, what is the pH of the solution at 25°C?

Calculate the pH of an acetate buffer made with 0.15 M acetic acid and 0.15 M sodium acetate after adding 10.0 mL of 0.10 M NaOH to 100.0 mL of the buffer. Assume Ka​ of acetic acid is 1.8 × 10−5.

At a certain temperature, the following reaction reaches equilibrium: N2(g)+3H2(g)⇌2NH3(g) At equilibrium in a 2.00 L container, the concentrations are: [N2​]=0.400M [H2​]=0.500M The equilibrium constant at this temperature is Kc = 0.040. What is the concentration of NH3 at equilibrium?

Formic acid, HCOOH, has a Ka value equal to ~1.8 x 10-4. A student is asked to prepare a buffer with a pH of 3.2 from a 0.05 M HCOOH and a 0.05 M NaCOOH solution. How many milliliters of the NaCOOH solution should they add to 15 mL of the HCOOH solution to make the buffer?

The rate constant for a reaction is 2.5 × 10⁻³ s⁻¹ at 298 K, and 7.5 × 10⁻³ s⁻¹ at 308 K.Calculate the activation energy (Eₐ) for the reaction in kJ/mol.

What is an elementary reaction?

In an acid-base titration, 22.13 mL of an NaOH solution are needed to neutralize 24.65 mL of a 0.1094 M HCl solution. What is the molarity of the NaOH solution?