How much dry solute would you take to prepare each of the following solutions from the dry solute and the solvent?
1. 116 g of 0.200 m NaNO3?
2. 116 g of 1.6 % NaNO3 solution by mass?
3. How much solvent would you take to prepare the solution in question 1?
4.How much solvent would you take to prepare the solution in question 2?
Q1:
Let mass of solute = x gm and mass of solvent would be (116-x)gm
Molality = mass of solute/molar mass × 1000/mass of solvent(in gm)
0.200 = (x/84.9947)×(1000/(116-x)) = 11.76544x/(116-x)
x = 1.9389 g
Mass of solute required = 1.94 g (answer)
Q2:
116 g of 1.6% NaNO3 by mass.
100g of solution has 1.6g of NaNO3
116g of solution has (1.6/100)×116g = 1.856g
Mass of solute required = 1.856g = 1.86g. (Answer)
Q3:
Mass of solvent = mass of solution - mass of solute
= 116g - 1.9389g = 114.06g
= 114.1g. (Answer)
Q4:
Mass of solvent = 116g - 1.856g = 114.144g
= 114.14 g. (Answer)
How much dry solute would you take to prepare each of the following solutions from the...
Describe how to prepare each solution from the dry solute and the solvent. Part A Part complete How much dry solute would you take to prepare 135 mL of 0.100 M NaNO3 ? Express your answer using three significant figures. -- Part B Part complete How much dry solute would you take to prepare123 g of 0.120 m NaNO3 ? Express your answer using three significant figures. -- msolute m s o l u t e = nothing gNaNO3 Part...
Explain how you would prepare each of the following solutions, using liquid stock hydrogen peroxide as the solute and saline as the solvent Section 3 Drug Dosage Calculations Review Set 27 plain how you would prepare each of the following solution as the solute and saline as the solvent. 1. 480 mL of strength for wound irrigation
13.54 Describe how you would prepare each of the following aque- ous solutions: (a) 1.50 L of 0.110 M (NH4)2SO4 solution, starting with solid (NH4)2SO4; (b) 225 g of a solution that is 0.65 m in Na2CO3, starting with the solid solute; (c) 1.20 L of a solution that is 15.0% Pb(NO3) 2 by mass (the density of the solution is 1.16 g/mL), starting with solid solute; (d) a 0.50 M solution of HCI that would just neutralize 5.5 g...
Calculate the grams of solute needed to prepare each of the following solutions. Part A 1.0 L of a 3.0 M NaOH solution Express your answer using two significant figures. IVO AP R O 2 ? g NaOH Submit Request Answer Part B 5.5 L of a 0.40 M CaCl2 solution Express your answer using two significant figures. OVO ACOM O a ? m= g CaCl2 Submit Request Answer Part 190 mL of a 2.75 M NaNO3 solution Express your...
How would you prepare the following solutions? Unless stated otherwise, assume that the solvent is purified water and that you will dissolve the solute in a lesser amount of solvent and then "bring the solution to volume". Show your math.
How would you prepare the following solutions? Unless stated otherwise, assume that the solvent is purified water and that you will dissolve the solute in a lesser amount of solvent and then "bring the solution to volume". Show your math.
Each week before you have chemistry lab, someone needs to prepare all the solutions you will use in your experiment. Suppose your experiment for next week calls for 0.500 M NaOH solution, 3.00 M NH4Cl solution, and 0.100 M Na3PO4 solution. Calculate the mass in grams for each solute that would be needed to prepare 8.00 L of each of the solutions. Calculate the mass, in grams, of solute present in each of the following solutions: a. 225 g of...
How many grams of solute would you use to prepare the following solutions? 1. 349.5 mL of 1.05 M NaOH 2. 1.35 L of 0.471 M glucose (C6H12O6)
Describe how you would prepare each of the following aqueous solutions, starting with solid KBr. A. 0.90 L of 1.4×10−2 M KBr B. 110 g of 0.160 m KBr C. 1.95 L of a solution that is 14.0 % KBr by mass (the density of the solution is 1.10 g/mL) D. a 0.130 M solution of KBr that contains just enough KBr to precipitate 16.0 g of AgBr from a solution containing 0.480 mol of AgNO3
Describe how you would prepare each of the following aqueous solutions, starting with solid KBr. 1] 0.70 L of 1.4×10−2 M KBr Express your answer using two significant figures. Enter your answers numerically separated by commas. 2] 120 g of 0.190 m KBr Enter your answers numerically separated by commas. 3] 1.70 L of a solution that is 14.0 % KBr by mass (the density of the solution is 1.10 g/mL) Enter your answers numerically separated by commas. 4] a...