What is the molarity of H3PO4 solution if 358 mL is completely titrated by 876 mL of 0.0102 M Ba(OH)2 solution?
"H_\n3\nP\nO_\n4\n(\na\nq\n)\n+\nB\na\n(\nO\nH\n)_\n2\n(\na\nq\n)\n\u2192\nB\na\nH\nP\nO_\n4\n(\na\nq\n)\n+\n2\nH_\n2\nO\n(\nl\n)"
Now moles of "Ba(OH)_2=0.0102 \\times876 \\times10^{-3} = 8.94 \\times 10^{-3} moles"
As the ratio of "Ba(OH)_2" and "H_3PO_4" is 1:1 so the moles of "H_3PO_4=8.94 \\times 10^{-3}"
Now Molarity of "H_3PO_4 =" "\\dfrac{moles}{volume(ml )}\\times1000"
"=" "\\dfrac{8.94\\times10^{-3}}{358} \\times 1000=0.025M"
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