If 0.25 mol of sodium phosphate is dissolved in 1 L of water, what are the concentrations of each ion? What is the total ion concentration?
If 0.25 mol of sodium phosphate is dissolved in 1 L of water, what are the...
In a 0.25 M aquous solution of sodium phosphate What is the total concentration of all ions?
three sets of solutions are made from stock solutions of sodium bromide, 0.0275 mol/L, and chlorine dissolved in water, 0.150 mol/L. Set one uses 2.00 mL of the NaBr and 8.00mL of the Cl2 solution. At the moment of mixing, calculate the concentrations of the bromide ion and the chlorine molecules.
Hard water often contains dissolved calcium ion and magnesium ions. One way to soften water is to add phosphate salts. The phosphate ion forms insoluble precipitates with calcium and magnesium ions, removing them from solution. Suppose that a solution is 5.5×10−2 M in calcium chloride and 9.5×10−2 M in magnesium nitrate. What mass of sodium phosphate would have to be added to 11.5 L of this solution to completely eliminate the hard water ions? (Assume complete reaction.)
7.00×10−3 mol of HBr are dissolved in water to make 15.0 L of solution. What is the concentration of hydroxide ions, [OH−], in this solution?
When dissolved in water, 1.0 mol of MgCl2 will dissociate into ____[A]____ mol of of Mg2+and ____[B]____ mol of Cl-. If you dissolved 1.0 mol of MgCl2 in water to make 1.0 L of this solution, the concentration would be ____[C]____ M, the osmolarity would be ____[D]____ osmol/L, the concentration of cations would be ____[E]____ Eq/L.
25.00 g of potassium hydrogen phosphate (K HPO4) is dissolved in enough water to make 125.0 mL of a solution with a density of 1.22 g/mL. What is the concentration of the solution in % (m/m). % (m/v). molarity, mosM and mEq/L of the potassium ion? Note: K2HPO4 has a molar mass of 174.2g/mole. What would be the final molarity of the above solution if you were to dilute it by adding 175 mL of water?
Question 17 0.5 pts 0.25 mol of solid glucose (C6H120) is dissolved in 100. mL of water, what is the (w/w%)-(3 SF) Question 18 0.5 pts What is the w/w% if 293.7 g is dissolved in 1.00 L of water to give a density 1.18 g/mL D Question 19 0.5 pts What is the concentration in V/V% for 250 mL of solution contains 13.1 mL of acetone. (3 SF)
The molar solubility of silver phosphate, Ag3PO4, is 4.68E-6 mol/L. (1) Express the solubility in units of grams per liter. (2) Calculate the concentration of silver ion in a saturated solution of silver phosphate. mol/L
A 1.20M solution of K3PO4 is prepared. What is the concentration of potassium ion in mol/L? What is the concentration of phosphate ion in mol/L?
The Solubility Product Constant for zinc phosphate is 9.1x10- If zinc phosphate is dissolved in water you can say that the equilibrium concentrations of zinc and phosphate ions are: A. High B. Moderate C. Low The solubility of zinc phosphate in water is: A. High B. Moderate C. Low Submit Answer Try Another Version 3 item attempts remaining