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Calculate [H3O+] 0.100 M NaNO2

Buffers- Common Ion effectIS this Correct Calculate the pH of a aqueous solution containing 0.15 M HNO2 and 0.20 M NaNO2 (aq).
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2. asked by Saira
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Calculate [H3O+]0.100 M NaNO2 and 5.00×10−2 M HNO2 so there's no Ka value for NaNO2, it can be ignored 5.6x10^-4 = x^2 /
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Sodium nitrite is prepared by a reaction of sodium nitrate and carbon: NaNO3 + C → NaNO2 + CO2 Calculate the masses of
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Section: Ionization expressions, Weak BasesUsing the equilibrium constants listed in your book, arrange the following .1 M
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2. asked by Chris
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How many grams of NaNO2 should be dissolved in 500cm3 solution of nitrous acid (HNO2) with concentration of 0.03mol/dm3 if we
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2. asked by Anonymous
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Calculate [H3O+] in the following solutions.1) 0.100 M NaNO2 and 5.00×10−2 M HNO2 2) 5.20×10−2 M HCl and 7.62×10−2 M
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2. asked by Lol
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What volumes of 0.46 M HNO2 and 0.54 M NaNO2 must be mixed to prepare 1.00 L of a solution buffered at pH = 3.40?a) HNO2 b)
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2. asked by justin
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Calculate the pH of 1.00L of a buffer that is 0.120M HNO2 and 0.150M NaNO2 before and after the addition of 1.00mL of 12.0M HCl
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2. asked by Amanda
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Calculate [H3O] in the following solutions.a)4.0×10−2M HCl and 8.0×10−2M HOCl b)0.105M NaNO2 and 5.00×10−2M HNO2
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2. asked by tomi
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Which of the following mixtures would result in buffered solutions when 1.0 L of each of the two solutions are mixed?a) 0.10 M
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2. asked by Saira
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