2NaOH + H2SO
4
Na2SO4 + 2H2O
Moles of NaOH = molarity×volume/1000
= 1×30/1000 = 0.03 moles
Moles of H2SO4 = 1×10/1000 = 0.01 moles
According to the reaction,
2 moles of NaOH require 1 mole H2SO4
0.03 moles of NaOH require 0.03/2 = 0.015 moles of H2SO4
Since we have less than this, hence H2SO4 is a limiting reagent.
According to the reaction,
1 mole H2SO4 give 1 mole Na2SO4
0.01 mole of H2SO4 give 0.01 moles of Na2SO4
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5 ml of 1M NaOH reacts with 10 ml of 1 M H2SO4 - how many moles of Na2SO4 are produced & what is the limiting reactant?
How many milliliters of 0.250 M NaOH are required to neutralize 55.0 mL of 0.300 M H2SO4? The balanced neutralization reaction is: H2SO4(aq) +2 NaOH(aq) → Na2SO4(aq)+2H2O(l).
when .0015 M of HCl reacts with .0035 M NaOH.
how do I get HCl as the limiting reactant?
HC # Results/Observations 1 Reaction Between Hydrochloric Acid and Sodium Hydroxide Table 1 ml LOM mol HCI ml 1.0M mol NaOH Temperature NaOHT change. "C 19. 10 0045 50L2012 .0005 22.4 #2 19.10.0 .004 10.09.11 .001 24.3 #3 1949350 -0035 15.020 Ốc DD15 265 #499 300 003 20.0 20.10 .002 27.3 #5 A5 2.0 .0025 25.0 20. 0 0025 2100 #6...
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