What volume of 18 M sulfuric acid must be used to prepare 2.00 L of 0.140 M H2SO4?
Volume of 18 M Solution = 15.6 ml or 0.0156 L
What volume of 18 M sulfuric acid must be used to prepare 2.00 L of 0.140...
What volume of 18.0 mol/L sulfuric acid must be used to prepare 15.5 L of 0.178 mol/L H2SO4
What volume of 18.0 M sulfuric acid must be used to prepare 15.5 L of 0.195 M sulfuric acid solution? O a. 168 ml O b.0.336 L O C. 168 L O d. 226 mL 923 m
162) Find the volume of 0.140 M sulfuric acid necessary to react completely with 71.0 g sodium hydroxide. Express your answer with the appropriate units.
Calculate the number of moles of solute in 2.00 L of 15.0 M H2SO4, concentrated sulfuric acid.
A stock solution of concentrated sulfuric acid, H2SO4, has a known concentration of 18.0M, What volume of concentrated sulfuric acid must be used to prepare 100.0ml, of 5.50M sulfuric acid solution? Select one: O a. 30.56ml O b. 0.235mL O c. 30.6ml O d. 327.3mL O e. 32.7mL
What volume of 18.0 M sulfuric acid must be diluted to 250.0 mL to afford a 0.55 M solution of sulfuric acid? (A) 3.1 mL (B) 4.5 ml (C) 7.6 mL (D) 31 ml
You need to make 2.00 L of a sulfuric acid solution that has a concentration of 0.103 M. If you are going to only use 25.0 mL of stock solution to make the dilution, what must the concentration of the stock solution be?
Enter your answer in the provided box. Calculate the volume of 11.7 M sulfuric acid that must be added to water to prepare 5.879 L of a 0.808 M solution.
Deterine the volume of 0.240 M KOH solution required to neutralize each sample of sulfuric acid. The neutralization reaction is: H2SO4(aq)+2KOH(aq)-->K2SO4(aq)+2H2O(L) a) 35mL of 0.240 M H2SO4 b) 175mL of 0.120 M H2SO4 c) 45mL of 0.115 M H2SO4
Calculate the milliliter of 2.00 M sulfuric acid needed completely neutralize 0.0500 L of 1.00 M of potassium hydroxide Answer: 12.5 mL