Question

How many milliliters of an aqueous solution of 0.152 M sodium phosphate is needed to obtain...

How many milliliters of an aqueous solution of 0.152 M sodium phosphate is needed to obtain 8.47 grams of the salt? mL

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
How many milliliters of an aqueous solution of 0.192 M iron(II) sulfate is needed to obtain...
How many milliliters of an aqueous solution of 0.192 M iron(II) sulfate is needed to obtain 7.68 grams of the salt?
How many milliliters of 5.5 M HCl solution are needed to obtain 0.14 mol of HCl?...
How many milliliters of 5.5 M HCl solution are needed to obtain 0.14 mol of HCl? Express the volume in milliliters to two significant digits How many moles of KBr are present in 140. mL of a 0.128 M solution? Express the amount in moles to three significant digits.
You need to make an aqueous solution of 0.162 M iron(II) sulfate for an experiment in...
You need to make an aqueous solution of 0.162 M iron(II) sulfate for an experiment in lab, using a 250 mL volumetric flask. How much solid iron(II) sulfate should you add? ___ grams How many milliliters of an aqueous solution of 0.207 M copper(II) acetate is needed to obtain 7.15 grams of the salt? ____mL In the laboratory you dissolve 24.2 g of lead nitrate in a volumetric flask and add water to a total volume of 125 . mL....
How many milliliters of 0.215 M FeCl3 solution are needed to react completely with 32.7 mL...
How many milliliters of 0.215 M FeCl3 solution are needed to react completely with 32.7 mL of 0.0509 M AgNO3 solution? The net ionic equation for the reaction is: Ag+(aq) + Cl-(aq) AgCl(s) mL of FeCl3: How many grams of AgCl will be formed?
(a) How many milliliters of 0.165 M HCl are needed to neutralize completely 35.0 mL of...
(a) How many milliliters of 0.165 M HCl are needed to neutralize completely 35.0 mL of 0.101 M Ba(OH)2 solution? ________ ml (b) How many milliliters of 2.50 M H2SO4 are needed to neutralize 50.0 g of NaOH? _________ mL (c) If 56.8 mL of BaCl2 solution is needed to precipitate all the sulfate in a 544 mg sample of Na2SO4 (forming BaSO4), what is the molarity of the solution? _________M (d) If 47.5 mL of 0.250 M HCl solution...
(a) How many milliliters of 0.165 M HCl are needed to neutralize completely 35.0 mL of...
(a) How many milliliters of 0.165 M HCl are needed to neutralize completely 35.0 mL of 0.101 M Ba(OH)2 solution? ______ml (b) How many milliliters of 3.50 M H2SO4 are needed to neutralize 75.0 g of NaOH? _______mL (c) If 55.8 mL of BaCl2 solution is needed to precipitate all the sulfate in a 544 mg sample of Na2SO4 (forming BaSO4), what is the molarity of the solution? ________M (d) If 47.5 mL of 0.375 M HCl solution is needed...
how many grams of sodium phosphate would you need to make 275 ml of 7.75 m...
how many grams of sodium phosphate would you need to make 275 ml of 7.75 m stock solution?
How many milliliters of a 0.221 M HCl solution are needed to neutralize 299 mL of...
How many milliliters of a 0.221 M HCl solution are needed to neutralize 299 mL of a 0.0459 M Ba(OH)2 solution?
How many milliliters of a .193 M HCl solution are needed to neutralize 221 mL of...
How many milliliters of a .193 M HCl solution are needed to neutralize 221 mL of a 0.0351 M Ba(OH)2 solution?
Calculate how many milliliters of 1 M NaOH will be needed to make 1 L of...
Calculate how many milliliters of 1 M NaOH will be needed to make 1 L of 0.1 M solution. Calculate how many grams of potassium acid phthalate (KHP, FW = 204.2 g/mol) will react with about 25 ml of the 0.1 M NaOH solution. The reaction is as follows: HKC8H4O4 + NaOH → H2O + NaKC8H4O4 Calculate how many mL of 1 M HCl is needed to make 1 L of 0.2 M HCl. HCl + NaOH → H2O +...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT