A solution is prepared by adding 1.0 mol of lithium nitrate. LINO3 to 1.00 L of water. Which of the following statement about the solution is correct?
The solution is neutral.
The solution is basic.
The solution is strongly acidic.
The solution is weakly acidic.
The values of Ka and Kb for the species in the solution must be known in order to make a prediction.
A solution is prepared by adding 1.0 mol of lithium nitrate. LINO3 to 1.00 L of water
A solution is prepared by adding 0.10 mol of lithium nitrate, LiNO_3 to 1.00 L of water. Which statement about the solution is correct? A)The solution is basic. B) The solution is C) The solution is weakly acidic. D) The solution is strongly acidic. E The values for K_a and K_b for the species in solution must be known before a prediction can be made. The pH of blood is 7.35. It is maintained in part by the buffer system...
A solution is made by adding 2.3 moles of Sr3(PO4)2 in 3.5L of water. Which of the following statements are true? The solution is strongly basic The solution is strongly acidic The solution is weakly basic The solution is weakly acidic The solution is neutral The Ka and Kb of the species added must be known Why would this not be weakly basic if the "roots" are Sr(OH)2, a strong base, and H3PO4, a weak acid? Do I have the...
A buffer is prepared by adding 1.00 L of 1.0 M HCl to 750 mL of 1.5 M NaHCOO. What is the pH of this buffer? Ka = 1.7
Calculate the pH of the solution made by adding 0.50 mol of HObr in 0.30 mol of KOBr to 1.00 L of water. The value of Ka for HObr is 2.0 * 10^-9
What is the pH of a buffer prepared by adding 6.0 mol of acetic acid and 1 mol of NaOH to water to make a 1.0-L solution? Ka for acetic acid is 1.75*10-5 and its pKa is 4.76.
A buffer is prepared by adding 0.15 mol of lactic acid, CH3CHOHCOOH, and 0.20 mol of sodium lactate, Na+CH3CHOHCOO - , to sufficient water to make 1.0 L of buffer solution. The Ka of lactic acid is 1.4 x 10 - 4. Calculate the pH of the buffer.
A solution was prepared with 0.346 mol of pyridinium fluoride (CH-NHF) and enough water to make a 1.00 L. Pyridine (CHșN) has a Kb = 1.70 x 10-9 and HF has a Ka = 6.30 x 10-4. Calculate the pH of the solution. pH =
A solution was prepared with 0.301 mol of pyridinium fluoride (C-H NHF) and enough water to make a 1.00 L. Pyridine ( CzH;N) has a Kb = 1.70 x 10-9 and HF has a Ka 6.30 x 10-4 = Calculate the pH of the solution. pH = Enter numeric value
1. Calculate the equilibrium concentrations of all species present and the pH of a solution obtained by adding 0.100 moles of solid NaOH to 1.00 L of 15.0 M NH3. Kb = 1.8 × 10–5 2. One mole of a weak acid HA was dissolved in 2.0 L of water. After the system had come to equilibrium, the concentration of HA was found to be 0.45 M. Calculate the Ka for this weak acid. 3. Calculate the pH of a...
Consider a solution prepared by dissolving 3.30g of barium hypochlorite salt in 0.660 L of water at 25 degrees C. (Assume solubility of the salt in water). Ka = 3.0x10^-8 1) Write and balance the reaction according to which the salt dissociates in water. Make sure to include correct phases. 2) Briefly explain which ions (Ba2+ or ClO- or both or maybe neither?) will hydrolyze. Write and balance any appropriate hydrolysis reaction(s). 3) The Solution is expected to be (Acidic,...