what is the mass of the HCl given:
volume of HCl: 100ml
Density: 1.017g/mol
what is the mass of the HCl given: volume of HCl: 100ml Density: 1.017g/mol
Concentrated hydrochloric acid (HCl) (molecular mass 36.5 g/mol) has a molarity of 3.6M. What volume of concentrated HCl would you need to add to prepare a 20% (w/v) solution of HCl with a final volume of 500 mL, I have calcualted that 3.6mol/L x 36.5g/mol =131.40g/L. Then to get the 100ml value and percentage: 131.40/1000 x 100 =13.14g/100ml therefore 13.14%. 20% of this would be 2.628g. Is this the answer?
Question 1: 1g of Copper wire is reacted to completion in 100mL of HCL. What concentration of CuCl2(aq) will be produced? Question 2: How many moles of H2(g) will be produced when 10g of Copper wire reacts with 100mL of 6M HCL(aq)? Here's what I already know... Balanced Reaction: Cu(s) + 2HCL(aq) --> CuCl2(aq) + H2(g) Atomic Mass of Cu: 63.5g/mol Formula mass of HCL: 36.5g/mol Formula Mass of CuCl2: 134.5g/mol Molecular Mass of H2: 2g/mol
Hess’s law lab data and calculations Data and Calculations NAME INSTRUCTOR mass of Mg volume HCI mass HCl(density of solution mass of solution + Mg initial temperature final temperature ΔΤ -1.05g/ml) oC oC oC ΔΗ, ( for 1 mole of Mg) kJ/mol Average ΔΗ3 kJ/mol o550 mass of Mgo volume HC mass HCl(density of solution- 1.05g/mL) 56 mass of solution +MgO initial temperature final temperature grams mL oC ec oC oC Ical ΔΙ Inn kJ/mol kJ/mol ΔΗ4 (for 1 mole...
What volume of a concentrated HCL , which is 36.0% HCL by mass and has a density of 1.179g/mL , should be used to make 5.10 L of an HCL solution with a pH of 1.5
What volume of a concentrated HCl solution, which is 36.0% HCl by mass and has a density of 1.179 g/mL, should be used to make 4.65 L of an HCl solution with a pH of 1.9?
What volume of a concentrated HCl solution, which is 36.0% HCl by mass and has a density of 1.179 g/mL, should be used to make 4.60 L of an HCl solution with a pH of 1.60? Express your answer to two significant figures and include the appropriate units.
What is the volume V of a sample of 2.00 mol of copper? The atomic mass of copper (Cu) is 63.5 g/mol, and the density of copper is 8.92×103kg/m3.
Please help with this problem, Thanks! *Extra Info given: NaOH molar mass= 40.00g/mol HCl molar mass= 34.46g/mol HCI molar mass = 36.46 g/mol /// VU 1. If 25.88 ml of a 0.435 M HCl solution was titrated with 0.726 M NaOH solution, how much of NaOH would be required to reach the equivalence point? In addition, what would be the pH at the equivalence point? GRAA.435APHI
What is the volume V of a sample of 2.90 mol of copper? The atomic mass of copper (Cu) is 63.5 g/mol, and the density of copper is 8.92×103kg/m3. Express your answer in cubic centimeters to 3 significant figures.
What is the pH of a 200ml solution of 0.25M HCl combined with a 100ml solution of 0.25 NaOH?