If water is present in the volumetric flask when transferring the H2SO4 solution from the pipette, the final concentration of H2SO4 will be diluted. This is because the water will mix with the H2SO4 solution, increasing the total volume in the flask without adding more H2SO4 molecules. As a result, the concentration of H2SO4 will be lower than intended.
To dilute the 3.5 M H2SO4 solution to 2 M, you need to add water. Use the formula M1V1 = M2V2, where M represents molarity and V represent volume. For this situation, you'll end up adding 75 ml of water to the initial 75 ml of 3.5 M H2SO4 solution to achieve a final 2 M concentration.
To prepare a 0.50 M solution using 8.0 M H2SO4, you would need to dilute the concentrated solution with water. Using the formula M1V1 = M2V2, where M1 is the initial concentration, V1 is the initial volume, M2 is the final concentration (0.50 M), and V2 is the final volume (200.0 mL), you can calculate the volume of 8.0 M H2SO4 needed. This would be around 1.25 mL.
To make 4.5 M H2SO4 from concentrated sulfuric acid (98% H2SO4), you would need to dilute it with water. Calculate the volume of concentrated sulfuric acid needed based on the final volume desired, then add water to reach the total volume. Always remember to add acid to water slowly and carefully to avoid splashing or overheating.
To prepare a 0.005 M solution of H2SO4 with pH 4, you can first calculate the concentration of H+ ions needed to achieve a pH of 4. Then, use the dissociation of H2SO4 to determine the amount of H2SO4 needed to provide that concentration of H+ ions. Finally, dilute the calculated amount of H2SO4 with water to reach the desired volume of the solution.
If water is present in the volumetric flask when transferring the H2SO4 solution from the pipette, the final concentration of H2SO4 will be diluted. This is because the water will mix with the H2SO4 solution, increasing the total volume in the flask without adding more H2SO4 molecules. As a result, the concentration of H2SO4 will be lower than intended.
To dilute the 3.5 M H2SO4 solution to 2 M, you need to add water. Use the formula M1V1 = M2V2, where M represents molarity and V represent volume. For this situation, you'll end up adding 75 ml of water to the initial 75 ml of 3.5 M H2SO4 solution to achieve a final 2 M concentration.
1 m = 10 dm
To prepare a 0.50 M solution using 8.0 M H2SO4, you would need to dilute the concentrated solution with water. Using the formula M1V1 = M2V2, where M1 is the initial concentration, V1 is the initial volume, M2 is the final concentration (0.50 M), and V2 is the final volume (200.0 mL), you can calculate the volume of 8.0 M H2SO4 needed. This would be around 1.25 mL.
fraction = 3/10 1 m = 100 cm 30 cm/1m = 30 cm/100 cm = 3/10
To make 4.5 M H2SO4 from concentrated sulfuric acid (98% H2SO4), you would need to dilute it with water. Calculate the volume of concentrated sulfuric acid needed based on the final volume desired, then add water to reach the total volume. Always remember to add acid to water slowly and carefully to avoid splashing or overheating.
To prepare a 0.005 M solution of H2SO4 with pH 4, you can first calculate the concentration of H+ ions needed to achieve a pH of 4. Then, use the dissociation of H2SO4 to determine the amount of H2SO4 needed to provide that concentration of H+ ions. Finally, dilute the calculated amount of H2SO4 with water to reach the desired volume of the solution.
Since 1 m = 10 dm, then 1 m 60 dm + 30 dm = 70 dm + 30 dm = 100 dm = 10m or 1 m 60 dm + 30 dm = 1m 90dm = 10 m.
The scale "4 cm = 1 m" is a factor of 1:25 (1/25th scale). 1m/.04m = 25
1m
1m = 100cm 990cm/100cm/m = 9.9m 9.9m > 1m, so 990cm > 1m
100cm = 1m 1 m = 100 cm