Question

In: Chemistry

i need to make a 2.0 mM NaPhytate ( 923.8 g/mol) solution in 100mM NaAcetate i...

i need to make a 2.0 mM NaPhytate ( 923.8 g/mol) solution in 100mM NaAcetate i need to make a 8.4 ml solution

Solutions

Expert Solution

Ans. It’s assumed that-

            I. Na-phytate and Na-acetate do not react/interfere with each other.

            II. Addition of Na-phytate to Na-acetate doesn’t change the volume.

            III. Both the solutes are completely soluble in water.

# Given, volume of solution = 8.4 mL = 0.0084 L

# Given, [Na-phytate] = 2.0 mM = 0.002 M                                 ; [1 mM = 0.001 M]

Now,

            Required moles of Na-phytate = [Na-phytate] x vol. of solution in liters

                                                            = 0.002 M x 0.0084 L

                                                            = 0.0000168 mol

            Required mass of Na-phytate = Required moles x Molar mass

                                                            = 0.0000168 mol x (923.8 g/ mol)

                                                            = 0.01551984 g = 0.01552 g

                                                            = 15.5198 mg

# Given, [Na-acetate] = 100 mM = 0.100 M                                ; [1 mM = 0.001 M]

Now,

            Required moles of Na-acetate = 0.100 M x 0.0084 L = 0.00084 mol

            Required mass of Na-acetate = 0.00084 mol x (82.034388 g/ mol) = 0.0689 g

# Preparation of solution:

Option 1: If 100 mM Na-acetate is available: Take 0.01552 g Na-phytate in a clean 10.0 mL test tube. Add 8.4 mL of 100.0 mM Na-acetate solution (see, assumption 2). It is you desired solution.

# Option 2: If 100 mM Na-acetate is not available: Prepare 100.0 mM Na-acetate solution by dissolving 0.0689 g Na-acetate in 8.4 mL deionized water.

To the above solution, add 0.01552 g Na-phytate. Mix well. It is the desired solution.


Related Solutions

A solution is 5.66 % by mass NH3 (MM 17.04 g/mol) in water (MM 18.02 g/mol)....
A solution is 5.66 % by mass NH3 (MM 17.04 g/mol) in water (MM 18.02 g/mol). The density of the resulting solution is 0.974 g/mL. What is the mole fraction, molarity and molality of NH3 in the solution?
A solution is 3.24 M NH3 (MM 17.04 g/mol) in water (MM 18.02 g/mol). The density...
A solution is 3.24 M NH3 (MM 17.04 g/mol) in water (MM 18.02 g/mol). The density of the resulting solution is 0.974 g/mL. What is the mole fraction, mass percent and molality of NH3 in the solution?
You are provided with a 0.1 mM solution of proflavine (MW: 209.25 g/mol), a 6 mM...
You are provided with a 0.1 mM solution of proflavine (MW: 209.25 g/mol), a 6 mM solution of DNA, and solid NaCl (MW: 58.44 g/mol). How many μL of the proflavine solution would you need to make a 25 mL of the following stock solution: 1 µM proflavine, 100 mM NaCl, and 60 µM DNA?
A solution has a 0.102 mole fraction of CaCl2 (MM 110.98 g/mol) in water (MM 18.02...
A solution has a 0.102 mole fraction of CaCl2 (MM 110.98 g/mol) in water (MM 18.02 g/mol). The density of the solution is 1.05 g/mL. What is the molality, mass percent and molarity of CaCl2 in the solution?
A 0.148-M solution of X (Mm = 177 g/mol) has a density of 1.156 g/ml. What...
A 0.148-M solution of X (Mm = 177 g/mol) has a density of 1.156 g/ml. What is the molality of X in the solution?
A 500 mL saturated solution of MgCO3 (MM = 84.3 g/mol) is reduced to 120 mL...
A 500 mL saturated solution of MgCO3 (MM = 84.3 g/mol) is reduced to 120 mL by evaporation. What mass of solid MgCO3 is formed? Ksp = 4.0 x 10-5 for MgCO3. EDIT: If ions can evaporate in water then the answer below is right. If not, this is how I solved the problem. MgCO3 dissolves at a 1:1 ratio, therefore Ksp=s2 and s=Ksp1/2 (or sqrt of Ksp) s = (4.0x10-5)1/2 = .00632 M Using the equation M1V1=M2V2 M1 =...
Making mixture solution: Cupric nitrate : wt = 241.60 g/mol SMS : wt= 250.278 g/mol I...
Making mixture solution: Cupric nitrate : wt = 241.60 g/mol SMS : wt= 250.278 g/mol I want to make the mixture of solution that has cupric nitrate constant concentration at 10E-5 M, but SMS concentration will run from 0 to 10E-4M So please help me make like 6 mixture solutions that have same concentration of cupric nitrate and SMS concentration run in that range. Thank you. Please show step by step
A stock solution of MgCl2 (MM=95.21g/mol) is prepared by dissolving 5.25g sample to make a 500.0ml...
A stock solution of MgCl2 (MM=95.21g/mol) is prepared by dissolving 5.25g sample to make a 500.0ml aqueous solution. If a 5.00ml aliquot diluted to 100.0ml, what is the molar concentration of this new MgCl2?
When 150.0 mL of a 0.200 M Ca(NO3)2 (MM = 164.088 g/mol) solution is added to...
When 150.0 mL of a 0.200 M Ca(NO3)2 (MM = 164.088 g/mol) solution is added to 200.0 mL of a 0.150 M K3PO4 (MM = 212.27 g/mol) solution, what mass of calcium phosphate (MM = 310.17 g/mol) will precipitate? a. 9.31 g b. 3.10 g c. 2.91 g d. 1.40 g e. 4.65 g
What mass of Cu(OH)2 (MM= 97.56 g/mol) will dissolve in ,500 L of a pH solution...
What mass of Cu(OH)2 (MM= 97.56 g/mol) will dissolve in ,500 L of a pH solution (Ksp=2.2*10 ^=20). In which solution is Cu(OH)2 most soluble and least soluble: A. .01 M NaCl, B. .01M CuCl2, C. .01 HCL, or D. .01NaOH.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT