Answer) This question can be solved by using,,
According to question,,
M1 = 18.0 M , V1 = _ mL , M2 = 0.55 M , V2 = 250.0 mL
So,
What volume of 18.0 M sulfuric acid must be diluted to 250.0 mL to afford a...
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
What volume of 0.673 M sucrose solution must be diluted with water to prepare 250.0 mL of 0.467 M sucrose solution?
calculate the concentration of sulfuric acid if 8.0 mL of 18.0 M H2SO4 is diluted to 600 mL
Sulfuric acid (250.0 mL) is titrated with 176.5 mL 2.4 M NaOH to an equivalence point (the point where all the sulfuric acid is exactly neutralized). 2 NaOH + H2SO4 → 2 H2O + Na2SO4 (a) How many moles of sulfuric acid were in the original 250.0 mL? (b) What was the concentration of sulfuric acid in the original 250.0 mL sample?
What volume (mL) of a concentrated solution of sodium hydroxide (6.00 M) must be diluted to 200.0 mL to make a 0.880 M solution of sodium hydroxide? Question 37 options: A) 50.0 B) 29.3 C) 176 D) 26.4 E) 2.64
What volume of 18.0 mol/L sulfuric acid must be used to prepare 15.5 L of 0.178 mol/L H2SO4
1.how many moles in 250.0 mLof a 0.15 M nitric acid solution? 2. what volume of base is required to reach the equivalence point in a titration of 25.00 mL of 0.20 M sulfuric acid with 0.35 M potassium hydroxide? with chemical equation.
In the laboratory, a student dilutes 26.4 mL of a 10.5 M nitric acid solution to a total volume of 250.0 mL. What is the concentration of the diluted solution? Concentration = How many milliliters of 11.6 M hydrochloric acid solution should be used to prepare 5.50 L of 0.100 M HCl? Interpret the following equation for a chemical reaction using the coefficients given: CO(g) + Cl2(g) →→ COC12(g) On the particulate level: of CO(g) reacts with — of Cl2(g)...
A chemist must prepare 250.0 ml of hydrochloric acid solution with a pH of 1.80 at 25°C. He will do this in three steps: Fila 250.0 ml. volumetric flask about halfway with distilled water. • Measure out a small volume of concentrated (6.0 M) stock hydrochloric acid solution and add it to the flask. . Fill the flask to the mark with distilled water, Calculate the volume of concentrated hydrochloric acid that the chemist must measure out in the second...
a) Calculate the final concentration when 25.0 mL of an 18.0 M HCl solution is diluted to 0.500 L. b) Calculate the volume required when an 8.50 M KOH solution is diluted to form 95.0 mL of a 0.500 M KOH solution