WebThe reaction is KHC 2 H 4 O 4 i 00 + NaOH (m 0 → NaKC 2 H 4 O 4 inen + H 2 O 60 You can tben calculate the molarity of your NaOH knowing the volume of NaOH. the mass of KHP and the molar mass of KHP The mole ratio of KHP to NaOH is 1:1. Therefore, at the equivalence point of this titration. WebMay 3, 2016 · Explanation: Clearly there is a 1:1 equivalence, and as a first step we calculate the number of moles of hydrochloric acid: 45.0 ×10−3 ⋅ L ×0.400 ⋅ mol ⋅ L−1 = 1.80 × 10−2 ⋅ mol hydrochloric acid. We find an equivalent molar quantity of sodium hydroxide: 1.80× 10−2 ⋅ mol 0.500 ⋅ mol ⋅ L−1 ×103 ⋅ mL ⋅ L−1 = 36.0 ⋅ mL.
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WebOct 23, 2012 · 1 answer 30mL of .1M NaOH has .03*.1 = .003 moles NaOH. so, it will take .003 moles of KHP to react with it. Convert moles to grams to get the mass. answered by Steve October 23, 2012 Answer this Question Still need help? You can or browse more chemistry... questions. WebCalculate the moles of KHP in flask #2. grams KHP Molar Mass of KHP (A2) 204.22 g/mol moles KHP %3D Cal .009 (A11) %3D NOR 204.22 g/mol Expert Solution Want to see the full answer? ordinary lover kb
Experiment 6: STANDARDIZATION OF A BASE; MASS …
WebFirst, calculate the number of moles of strong base required to reach the equivalence point of the titration. Then, using the mole ratio from the balanced neutralization equation, … WebMar 8, 2016 · This tells you that at you can reach the equivalence point by reacting equal number of moles of KHP and of NaOH. You start with 0.5100 g of KHP. To get the … WebKHP (aq) + NaOH (aq) >> KNaP + H20 They react in a 1 to 1 ratio 1.390g KHP x ..1 mole KHP/204.2234 g KHP =6.806x10^-3 6.806x10-3 moles of KHP. Since you have a 1 to 1 ratio you have 6.806x10-3 moles of NaOH Now simply divide the number of moles by the volume titrated in liters. 6.806x10-3/ 22.3 mL * (1 L/100 mL) --> 0.02165L = 0.3144M ordinary low water mark california