How much water, in liters, must be added to 0.5 L of 6 M HCl to make it 2 M?

A. 0.33
B. 0.5
C. 1
D. 1.5
E. 2

How many liters of 0.2805 M C6H12O6(aq) contain 1.000 g of C6H12O6? a) 0.001557 L\tb) 0.01979 L\tc) 0.2805 L\td) 3.565 L\te) 50.5 L
2.\tIf 5.15 g Fe(NO3)3 is dissolved in enough water to make exactly 150.0 mL of solution, what is the molar concentration of nitrate ion? a) 0.00319 M\tb) 0.0343 M\tc) 0.142 M\td) 0.313 M\te) 0.426 M
3.\tWhat is the mass of sodium iodide in 50.0 mL of 2.63  10-2 M NaI(aq)? a) 0.00132 g\tb) 0.00877 g\tc) 0.0788 g\td) 0.197 g\te) 78.8 g
4.\tIf 25.00 mL of 4.50 M NaOH(aq) is diluted with water to a volume of 750.0 mL, what is the molarity of the diluted NaOH(aq)? a) 0.0333 M\tb) 0.150 M\tc) 0.155 M\td) 6.67 M\te) 1.35 × 103 M
5.\tWhat volume of 0.15 M HCl(aq) must be diluted to make 2.0 L of 0.050 M HCl(aq)? a) 0.015 L\tb) 0.10 L\tc) 0.30 L\td) 0.67 L\te) 6.0 L
6.\tWhat is the pH of 0.51 M HCl(aq)? a) -0.29\tb) 0.29\tc) 0.31\td) 0.51\te) 0.67
7.\tThe pH of an aqueous NaOH solution is 13.17. What is the hydrogen ion concentration of this solution? a) 6.8 × 10-14 M\tb) 1.9 × 10-6 M\tc) 0.89 M\td) 1.1 M\te) 1. 5 × 1013 M
8.\tThe pH of a vinegar solution is 4.15. What is the H3O+ concentration of the solution? a) 7.1 × 10-5 M\tb) 1.6 × 10-2 M\tc) 0.62 M\td) 1.4 M\te) 1.4 × 104 M
9.\tAn aqueous nitric acid solution has a pH of 1.15. What mass of HNO3 is present in 2.0 L of this solution? a) 0.071 g\tb) 0.14 g\tc) 2.2 g\td) 4.5 g\te) 8.9 g
10.\tIron reacts with hydrochloric acid. Fe(s) + 2 HCl(aq) → FeCl2(aq) + H2(g) What volume of 2.55 M HCl(aq) will react with 35.0 g Fe(s)? a) 0.246 L\tb) 0.492 L\tc) 1.60 L\td) 3.20 L\te) 27.5 L
11. What volume of 0.200 M Na2SO4(aq) will completely react with 50.0 mL of 0.135 M Ba(NO3)2(aq)? Na2SO4(aq) + Ba(NO3)2(aq) → BaSO4(s) + 2 NaNO3(aq) a) 33.8 mL\tb) 67.5 mL\tc) 74.1 mL\td) 148 mL\te) 540. mL
12.\tA mass of 0.4113 g of an unknown acid, HA, is titrated with NaOH. If the acid reacts with 28.10 mL of 0.1055 M NaOH(aq), what is the molar mass of the acid? a) 2.965 × 10-3 g/mol b) 9.128 g/mol c) 138.7 g/mol d) 337.3 g/mol e) 820.7 g/mol
13.\tA 25.00 mL sample of KOH is titrated with 21.83 mL of 0.2120 M HCl(aq). What is the concentration of the KOH solution? a) 0.0006720 M\tb) 0.002574 M\tc) 0.1851 M\td) 0.2428 M\te) 4.119 M

Answered by Anonymous | 2024-06-10

To dilute 0.5 L of 6 M HCl to 2 M, you will need to add 1.0 L of water to the solution. This is calculated using the dilution formula, leading to a final volume of 1.5 L. The required amount of water to add is the difference between the final volume and the initial volume, which is 1.0 L.
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Answered by Anonymous | 2024-12-20