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Chemistry
Acid-base reactions
Concentration calculation
The neutralization of 27.3 mL of an unknown concentration H2SO4 solution requires 72.2 mL of 0.12 M LiOH solution. What is the concentration of the H2SO4 solution (in M)?
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The neutralization of 27.3 mL of an unknown concentration H2SO4 solution requires 72.2 mL of 0.12 M LiOH solution. What is the
Top answer:
Na*Va=Nb*Vb The titration equation: if you do not know it, learn it. 2*Ma*27.3=1*.12(72.2) solve for
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The neutralization of 27.3 mL of an unknown concentration H2SO4 solution requires 72.2 mL of 0.12 M LiOH solution. What is the
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see the last post you did.
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The titration of 25.0 mL of an unknown concentration H2SO4 solution requires 83.6 mL of 0.12 M LiOH
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Ah scratch my last answer forgot that the mole ratio is 1:2 so you have to divide your M2V2 answer
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See your later posts.
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A 15.0 ml sample of an unknown HClO4 solution requires 50.3 ml if 0.101 M NaOH for complete neutralization.
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See your post above.
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A 15.0 ml sample of an unknown HClO4 solution requires 50.3 ml if 0.101 M NaOH for complete neutralization.
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moles NaOH = M x L = ? Look at the equation; it is 1:1, therefore, moles HClO4 = moles NaOH The M
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moles NaOH = M x L = ?? Look at the equation and use the coefficients to convert moles NaOH to moles
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A 27.4 mL sample of an unknown HClO4 solution requires 45.4 mL of 0.101 M NaOH for complete neutralization. What was the
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To determine the concentration of the unknown HClO4 solution, you need to use the stoichiometry of
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The titration of 25.0 mL of an unknown concentration H2SO4 solution requires 83.6 mL of 0.12 M LiOH solution. What is the
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H2SO4 + 2LiOH ==> Li2SO4 + 2H2O mols LiOH = M x L = ? mols H2SO4 = 1/2 that. M H2SO4 = mols H2SO4/L
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Write the balanced neutralization reaction between H2SO4 and KOH in aq. solution.
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2KOH + H2SO4 ==> K2SO4 + 2H2O Just another LR problem. You can ALWAYS spot LR problems because
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