A solution that has reached equilibrium and has undissolved solute remaining in the solution must be...
3. A solution is at pH 8.35 and has reached equilibrium with the atmosphere. (a) How much H2SO4 (mol/L) must be added to lower the pH to 6.0, if no gas/liquid exchange occurs? (b) Repeat part (a) if the solution remains in equilibrium with the atmosphere as the acid is added
An aqueous solution has a mole fraction of solute of (3.660x10^-2). The density of the solution is (1.20x10^0) g/mL and the solute has a molar mass of (8.3800x10^1) g/mol. What is the Molarity of solute of this solution? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 Answer
When the solution above has reached equilibrium, what effect would adding more Mg2+ have? Adding more F-? Why is it that NO MORE PRODUCT forms when more MgF2 is added to the solution at equilibrium?
Help with 13 Solution B has greater solute (solute "solute particles") concentration than does solution A. Solution A is hypoosmotic to Solution B. 13. You are instructed to make one liter of 150 mM of NaCI. Given the salt (NaCl) and equipment needed for weighing and measuring volumes, tell exactly how you would make this solution. (show all calculations). What is the osmolarity of this solution?
What are the equilibrium concentrations of all the solute species in a 0.99 M solution of propanoic acid, HC3H5O2? (a) [H3O+], M; (b) [OH-], M; (c) [CH3CH2COOH], M; (d) What is the pH of the solution? For CH3CH2COOH, Ka = 1.34 x 10-5.
1e. An aqueous solution has a mole fraction of solute of (4.73x10^-2). The density of the solution is (1.1400x10^0) g/mL and the solute has a molar mass of (8.020x10^1) g/mol. What is the Molarity of solute of this solution? 1f. At an unknown temperature a solution made of (7.740x10^0) g of a non-volatile solute dissolved in 100.0 g of water has a vapor pressure of (5.51x10^1) mm Hg. What is the vapor pressure of pure water (in mm Hg) at...
Answer QUESTION 5 Describe what happens at the molecular level once equilibrium is reached--that is, once the solution is saturated with Cu(IO_3)_2. Why must some solid remain in contact with a solution of a sparingly soluble salt in order to ensure equilibrium? Describe how you are going to calculate the [Cu^2+] for the saturated solution of copper iodate once you know the absorbance value of the copper ion. How will you use this concentration to find the K_sp value for...
What are the equilibrium concentrations of all the solute species in a 1.1 M solution of cyanic acid, HOCN? (a) [H30+], M; (b) (OH), M; (c) [HOCN), M; (d) What is the pH of the solution? For HOCN, Ka = 3.5 x 10-4. (a) M (b) M (c) M (d)
Enter your answer in the provided box. A solution of 1.55 g of solute dissolved in 25.0 mL of H20 at 25°C has a boiling point of 100.850°C. What is the molar mass of the solute if it is a nonvolatile nonelectrolyte and the solution behaves ideally (d of H20 at 25°C = 0.997 g/mL)? g/mol
Imagine a reaction that has reached equilibrium and in which the forward reaction at equilibrium is found to be 8.1 x10-5 Trls, what do you predict can be the rate of the reve -1 8.1 x 105 ak- b.k = 8.1x10 1 ck= -5 8.1 x 10- d. K- 1.8 x 10-5