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How much H2SO4 is needed to prepare 2000ml of 1.25H2SO4 from 98 ww H2SO4?
You need 252 g sulfuric acid.
Find volume of sulphuric acid of concentration 32 percent weight and density 1.531 gram per liter diluted to 5.8 liter to be 1.5 molar?
Initially, the mass of H2SO4 required to prepare 5.8 liters of 1.5 molar solution should be calculated. Number of moles present in 5.8 L of 1.5 molar solution = 1.5 mol L-1 x 5.8 L= 8.7 molMolar mass of H2SO4 = 98 g mol-1Therefore, mass of H2SO4 in the above solution = 8.7 mol x 98 g mol-1= 852.6 gMass of H2SO4 in the original solution per litre = 1.531 g x 32/100= 0.48992 gVolume of sulphuric acid required to prepare 1.5 molar solution = 852.6 g/0.48992 g = 1740.3 L
If 36.0 mL of a 0.158 M NaOH solution is required to titrate 24.0 mL of a solution of H2SO4 what is the molarity of the H2SO4 solution H2SO4(aq) plus 2NaOH(aq) 2H2O(l) plus Na2SO4(aq)?
I think you just use C1V1 = C2V2 , but don't forget the stoichiometric ratio of1 NaOH 0.5 H2SO4NaOH:C1 = .1650 mol/LV1 = 26.48 mLH2SO4:C2 = ? (mol/L of H2SO4)V2 = 28.22 mL26.49 x .1650 (mmoles of OH-) = 2 * C2 x 28.22 (mmoles of H+ from H2SO4) =C2 = 0.5 * 0.1548848335 = 0.07744 (mol/L H2SO4)
Which gas can be smelled when H2SO4 is added to copper chloride solution?
The chemical reaction is:CuCl2 + H2SO4 = CuSO4 + 2 HCl(g)The gas is hydrogen chloride.
How many grams of sulfuric acid H2SO4 are in 45.0 ml of a 6.5 M solution?
This solution contain 2,89 g sulfuric acid.
How will you make solution for ph4 of 0.005 normal h2so4?
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.
What is the number of moles os H2SO4 in 100mL of 12M H2SO4 solution?
To find the number of moles of H2SO4 in 100 mL of 12M H2SO4 solution, you first need to convert the volume to liters, which is 0.1 L. Then, you multiply the volume in liters by the molarity to get the moles of H2SO4. So, 0.1 L * 12 mol/L = 1.2 moles of H2SO4.
Martha has a large amount of 1.25 m H2SO4 in her lab she needs 36 grams of H2SO4 for a chemical reaction she wants to perform how many liters of the solution should she use?
To find the volume needed, you can use the formula: Volume of solution (in liters) = mass of solute (in grams) / concentration of solution (in g/L) First, convert the concentration of 1.25 M H2SO4 to g/L by multiplying by the molar mass of H2SO4 (98.08 g/mol). This gives 122.6 g/L. Then, plug in the values: 36 g / 122.6 g/L ≈ 0.29 L. So, Martha should use approximately 0.29 liters of the 1.25 M H2SO4 solution.
What is the total number of moles of H2SO4 needed to prepare 5.0 liters of a 2.0 M solution of H2SO4?
To find the total number of moles needed, use the formula n = M x V, where n is the number of moles, M is the molarity, and V is the volume in liters. Thus, n = 2.0 mol/L x 5.0 L = 10 moles of H2SO4 are needed.
What volume (in liters) of a 1.9 M NaOH solution would neutralize 7.2 moles of H2SO4 (diprotic)?
To neutralize 1 mole of diprotic acid (H2SO4), you need 2 moles of NaOH. Therefore, to neutralize 7.2 moles of H2SO4, you would need 14.4 moles of NaOH. Using the formula M = mol/L, where M is the molarity, mol is the amount of solute in moles, and L is the volume in liters, you can calculate the volume of the 1.9 M NaOH solution needed as 7.57 liters.
How do you prepare 2.5N h2so4?
how 2.5N H2SO4 prepared from concentrated H2SO4
How can you prepare 1N H2SO4 from H2SO4 95 percent?
To prepare 1N H2SO4 from 95% H2SO4, you would first need to dilute the 95% H2SO4 with water by adding the appropriate amount of water to achieve the desired concentration. To calculate the volume of 95% H2SO4 needed to make 1N solution, you need to use the formula: (Normality of stock solution) * (Volume of stock solution) = (Normality of diluted solution) * (Volume of diluted solution). Adjust the volumes accordingly to prepare the desired 1N solution.
Moles of H2SO4 in 20 ml of 4M solution?
To find the moles of H2SO4 in a 20 ml of 4M solution, use the formula: Moles = Molarity x Volume (in liters). First, convert 20 ml to liters (20 ml = 0.02 L). Then, multiply the molarity (4 mol/L) by the volume (0.02 L) to find the moles of H2SO4, which is 0.08 moles.
What volume of 6.40 m h2so4 is needed to prepare 455.0ml of a solution that is 0.700m in h2so4?
To find the volume of 6.40 M H2SO4 needed to prepare a solution that is 0.700 M, you can use the formula: M1V1 = M2V2, where M1 is the initial concentration, V1 is the initial volume, M2 is the final concentration, and V2 is the final volume. Rearranging the formula, V1 = (M2*V2) / M1 gives you the volume: V1 = (0.700 * 455.0) / 6.40 = 49.53 ml. You would need 49.53 ml of the 6.40 M H2SO4 solution to prepare 455.0 ml of a 0.700 M H2SO4 solution.
How do you standardize 1N H2SO4 with a KHP?
To standardize 1N H2SO4 with KHP, you would first prepare a solution of KHP of known concentration. Then, titrate the KHP solution with the 1N H2SO4 solution until the endpoint is reached. The volume of H2SO4 used in the titration can then be used to calculate the exact concentration of the H2SO4 solution.
A chemist has 2 solutions of h2so4 One 40 concentration and the other 25 solution How many liters must be mixed to make 129 liters of 31 solution?
For a detailed answer visit: algebra.com/algebra/homework/word/mixtures/Mixture_Word_Problems.faq.question.786696.html
What mass of h2so4 would required to prepare 750 ml of a 0.15m h2so4 solution?
To calculate the mass of H2SO4 required, first calculate the number of moles needed using the formula: moles = molarity x volume (in liters). Then, multiply the moles by the molar mass of H2SO4 (98.08 g/mol) to find the mass. moles = 0.15 mol/L x 0.75 L = 0.1125 mol mass = 0.1125 mol x 98.08 g/mol ≈ 11.04 g of H2SO4.
