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How would you prepare 1000.0ml of 0.600M NaOH solution starting from concentration of 1.000M.
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How would you prepare 1000.0ml of 0.600M NaOH solution starting from concentration of 1.000M
Top answer:
I would use the dilution formula. c1v1 = c2v2 1M x V1 = 0.600 x 1000 mL Solve for V1 in mL; place
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Can someone please explain this problem step by step.
How would you prepare 1000.0ml of 0.600M NaOH solution starting from
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The dilution formula is c1v1 = c2v2 1.000*v = 0.600*1000 v = 600. Take 600 mL of the 1.000M and
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Volume of stock solution
a. 5.0mL b.10.0mL c.15.0mL d.20.0mL Prepare 25mL of each of the four different dilute solution
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NiCl2(aq) + 2NaOH(aq) → Ni(OH)2(s) + 2NaCl(aq) First get the number of moles of NaOH. Recall that
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what is the molar concentration of h2so4 solution is 2.0ml of which is completely neutralized by 45.0ml of 0.115 mol/L NaOH
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H2SO4 + 2NaOH ==> 2H2O + Na2SO4 mols NaOH = M x L = ? Note that mols H2SO4 = 1/2 mols NaOH Then M
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A 15.0mL solution of H2SO3 is neutralized by 12.0mL of a standardized 1.00M NaOH solution. What is the concentration of the
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H2SO3 + 2NaOH ==> Na2SO3 + 2H2O mols NaOH = M x L = ? Convert mols NaOH to mols H2SO3 so mols H2SO3
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If 20.0mL of .2019M HCI requires 39.63mL of a NaOH solution for complete neutralization, what is the concentration of the NaOH
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HCl + NaOH ==> NaCl + H2O mols HCl used = L x M = 0.0200 L x 0.2019 M = ?? mols NaOH (from the
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what is the concentration of hydrogen ion in a 0.1M solution of sodium hydroxide(NaOH)?
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To calculate the concentration of hydrogen ions (H+) in a 0.1 M solution of sodium hydroxide (NaOH),
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Describe how you would prepare 25.0ml of a 1.00 M NaOH solution.
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To prepare 25.0 ml of a 1.00 M NaOH solution, you will need to follow a step-by-step procedure.
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