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a solution is made by mixing 14.5g of NaOH and 72.0 mL of 0.250 M HNO3
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Concentration of OH- left in a solution made by mixing 16.0 g of NaOH and 80.0 mL of 0.170M HNO3?
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HNO3 + NaOH ==> NaNO3 + H2O moles HNO3 = M x L = 0.0136 moles NaOH = g/molar mass = 16/40 = 0.4 So
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A solution is made by mixing 12.0 g of NaOH and 75.0 ml of 0.200 M HNO3
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calculate the moles of each reactant. The smaller of the two is how much reacted.
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A solution is made by mixing 12.0 g of NaOH and 75.0 ml of 0.200 M HNO3
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NaOH(aq) + HNO3(aq) ==> NaNO3(aq) + H2O(l)
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What is the pH of the solution when 50.00 mL of 0.250 M HNO3, nitric acid, has been treated with 25.00 mL of 0.400 M NaOH?
Below
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Alex, you got me. I don't know. It looks ok to me. USUALLY it is a matter of an incorrect number of
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I have 5.217 which rounds to 5.22. Good work. I have pH = 4.74 + log (12/4) You may not have used
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pH of a Buffered Solution
How to calculate ph of this solution? A solution made by mixing 120.00 mL of 0.950 M HNO2 with 55.00 mL
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