Homework Answers
Since HCl is a strong acid and KOH is a strong base, hence it will dissociate completely into solution
The balanced reaction will be
HCl + KOH ------------- KCl + H2O
Number of moles of HCl = Number of moles of KOH
Molarity of HCl * Volume of HCl (in L) = Molarity of KOH * Volume of KOH (in L)
Molarity of HCl * 25.0/1000 = 0.125 * 43.6/1000
Molarity of HCl = (0.125 * 43.6)/(25.0) = 0.218 M
Note - Post any doubts/queries in comments section.
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68.5 mL of a HNO3 solution with unknown concentration is
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Exercise 14.47 Four solutions of unknown HCl concentration are titrated with solutions of NaOH. The following...
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answer (2)
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68.5 mL of a HNO3 solution with unknown concentration is
titrated with 0.150 M KOH solution. The end point is reached after
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solution ?
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answer (2)
2. Suppose that you used a known concentration (0.8442 M) of Ca(OH)2 to determine the concentration of an unknown HBr solution. If it takes 12.88 mL of the Ca(OH)2 solution to titrate 15.00 mL of the unknown HBr solution, what is the molarity of the HBr? 1. A solid diprotic weak acid, H2A (molecular weight = 128.9 g/mol) is used to standardize a KOH solution. When 0.4228 g of the acid is dissolved in 40.0 mL of water...
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both Cancentrations is in the Solution. 4. I1300 ml of o.500 M KOH is nedt eutralize 10.0 ml of an unknown concentration HCI, what is molarity of the HC1? 6 M . A 10.0-mL sample of HCl is titrated using 27.50-mL of a 1.50 M NaOH. Calculate (a) the molar concentration of the hydrochloric acid and (b) the mass/volume percent concentration of hydrochloric acid. 160
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