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Calculate the pH when 75.20 mL of 0.114 M HCl is titrated with 0 ml of 0.108 M NaOH
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Calculate the pH when 75.20 mL of 0.114 M HCl is titrated with 0 ml of 0.108 M NaOH
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The pH at what point?
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if 50.0 mLs of HCl of unknown concentration is titrated to neutrality with 90.0 mL of .650 M NaOH. calculate the molarity of the
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NaOH and HCl react 1:1 so you can use the simplified equation mL NaOH + M NaOH = mL HCl x M HCl
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if 50.0 mLs of HCl of unknown concentration is titrated to neutrality with 90.0 mL of .650 M NaOH. calculate the molarity of the
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To calculate the molarity of the HCl solution, we need to use the concept of stoichiometry and the
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A25.0mL sample of 0.1MNH3 is titrated with 0.1M HCl.
A . calculate the pH value of the solution after the following volume of
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A. 0.00 mL: pH = 11.00 5.00 mL: pH = 9.00 10.00 mL: pH = 7.00 15.00 mL: pH = 5.00 20.00 mL: pH =
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Consider the following reaction.
2 HCl(aq) + Ba(OH)2(aq) BaCl2(aq) + 2 H2O(l) ΔH = -118 kJ Calculate the heat when 114.8 mL of
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An antacid tablet weighing 1.462 grams was dissolbed in 25mL of 0.8M HCl and diluted with water. The excess HCl was titrated
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1) mmoles HCl added to tablet = mL x M = ?? 2) mmoles NaOH added to HCl = mL x M = ?? 3) #1-#2=#3
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An antacid tablet weighing 1.462 grams was dissolbed in 25mL of 0.8M HCl and diluted with water. The excess HCl was titrated
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A 10.0 mL solution of 0.300 M NH3 is titrated with a 0.100 M HCl solution. Calculate the pH after the addition of 20.0 mL of the
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millimoles NH3 = 10 x 0.3 = 3 mmols HCl = 20 x 0.1 = 2 NH3 + HCl => NH4Cl So you have 2 mmols NH4^+
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50gm of a sample of ca(oh)s is dissolved in 50ml of 0.5N hcl solution. The excess of hcl was titrated with 0.3N -naoh. The
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To calculate the percentage purity of Ca(OH)2, we need to determine the number of moles of Ca(OH)2
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A 10.0-mL solution of 0.300 M NH3 is titrated with a 0.100 M HCl solution. Calculate the pH after the following additions of the
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Actually I figured out a, b, c, and d but I can't figure out e. What do you do if HCl is in excess?
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