The amount of potassium phosphate in the solution is 1.27 M * 0.343 L = 0.43561 moles.
The chemical formula of potassium phosphate is K3PO4, so there is three times as many moles of potassium as there are moles of potassium phoshate in the molecule:
0.43561 * 3 = 1.30683
Answer: 1.31 moles
Molarity = moles of solute/Liters of solution ( 25 ml = 0.025 Liters ) 1.5 M KBr = moles KBr/0.025 Liters = 0.038 moles potassium bromide ------------------
Molarity = moles of solute/Liters of solution ( 75.0 ml = 0.075 Liters ) Algebraically manipulate, moles of solute = Liters of solution * Molarity Moles KMnO4 = (0.075 Liters)(0.0950 M) = 7.13 X 10 -3 moles KMnO4 ------------------------------------
0.1 moles
None, unless there is metallic potassium in the reaction mixture. Assuming excess potassium metal is present then 14 moles of KBr can be produced. 7BaBr2 + excess potassium -----> 14KBr + 7 Ba
Molarity = moles of solute/Liters of solution (40 ml = 0.04 Liters) algebraically manipulated, Moles of solute = Liters of solution * Molarity Moles HCl = (0.04 Liters)(0.035 M) = 0.0014 moles HCl ==============
0,052 moles
there are two moles produced in potassium nitrate.
Molarity = moles of solute/Liters of solution ( 25 ml = 0.025 Liters ) 1.5 M KBr = moles KBr/0.025 Liters = 0.038 moles potassium bromide ------------------
Molarity = moles of solute/Liters of solution ( 75.0 ml = 0.075 Liters ) Algebraically manipulate, moles of solute = Liters of solution * Molarity Moles KMnO4 = (0.075 Liters)(0.0950 M) = 7.13 X 10 -3 moles KMnO4 ------------------------------------
0.1 moles
None, unless there is metallic potassium in the reaction mixture. Assuming excess potassium metal is present then 14 moles of KBr can be produced. 7BaBr2 + excess potassium -----> 14KBr + 7 Ba
Ten milliliters is a hundredth of a liter. So in a two molar solution, you would have .02 moles in 10 ml.
The answer is 0,o276 moles.
8.42 grams of KOH is equal to 0.15 moles. If the solution has a molarity of 2.26 moles per liter, then there are 66.4 milliliters of solution.
Find moles potassium iodide first.2.41 grams KI (1 mole KI/166 grams) = 0.01452 moles KIMolarity = moles of solute/Liters of solution ( 100 ml = 0.1 Liters )Molarity = 0.01452 moles KI/0.1 Liters= 0.145 M KI solution================
Molarity = moles of solute/liters of solution ( 300 ml = 0.300 liter ) 0.250 molar KOH = moles KOH/0.300 liters = 0.075 moles KOH
Molarity = moles of solute/Liters of solution (40 ml = 0.04 Liters) algebraically manipulated, Moles of solute = Liters of solution * Molarity Moles HCl = (0.04 Liters)(0.035 M) = 0.0014 moles HCl ==============