Can you please show work, a detailed step by step on how to solve the problems.
ID: 982820 • Letter: C
Question
Can you please show work, a detailed step by step on how to solve the problems. Thank you! How many grams of sodium hydroxide (NaOH) should be added to 450.0 g of water to prepare a 1.750 m NaOH(aq) solution? A 1.400 m H_2SO_4(aq) solution contains how many grams of H_2SO_4 dissolved per every 100.0 g of water? A solution is prepared by dissolving 4.30 g of potassium nitrate (KNO_3) in 50.0 g of water. What is the % mass of KNO_3? What is the molality of the solution? What is the mole fraction of KNO_3 in the solution? At 15.0 degree C, an aqueous solution that is 35.0 % sucrose (C_12H_22O_11) by mass has a density of 1.145 g/mL. What is the molality of the solution? What is the molarity of the solution? What is the mole fraction of sucrose in the solution? At 20.0 degree C, a 7.816 m HNO_3 aqueous solution has a density of 1.200 g/mL. What is the molarity of the solution? What is the mole fraction of HNO_3 in the solution? What is the % mass of HNO_3? At 20.0 degree C, a 2.594 MFeCl_3 aqueous solution has a density of 1.315 g/mL. What is the molality of the solution? What is the mole fraction of FeCl_3 in the solution? What is the % mass of FeCl_3?Explanation / Answer
|)
grams of NAOH
m = 450 g of water
V = 450 ml (assume 1 g/ml)
m of watter = 0.45 KG
m = mol/kg solvent
m = 1.75
1.75 = mol/kg
mol = 1.75*0.45 = 0.7875 mol naoh needed
mass = mol*MW = 0.7875*40 = 31.5 g of NaOH
b)
m = 1.4 m H2SO4
if mass solvent = 100 g = 0.1 kg
mol = m*kg = 1.4*0.1 = 0.14 mol of H2SO4
mass = mol*MW = 98*0.14 = 13.72 g of H2SO4
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