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Calculate the pOH of an aqueous solution of 146.6 ml of 0.000625 M HBr(aq) after dilution to 850 ml.
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Calculate the pOH of an aqueous solution of 146.6 ml of 0.000625 M HBr(aq) after dilution to 850 ml.
Top answer:
To calculate the pOH of the aqueous solution, we need to know the concentration of hydroxide ions
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Calculate the pOH of an aqueous solution of 146.6 ml of 0.000625 M HBr(aq) after dilution to 850 ml.
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(HBr) diluted = 0.000625 x (146.6/860) = about 1.08E-4 pH = -log(H^+) = -log(HBr) since HBr is a
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Calculate the pH and pOH of each of the following aqueous solutions of strong acd or base:
(a) 0.010 M HNO3(aq) (b) ) 1.0 x 10-3M
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Here is how you do a and b. a. HNO3 is a strong acid; i.e., it ionizes 100%. Therefore, HNO3 ==> H^+
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Calculate the pH and the pOH of an aqueous solution that is 0.025 M in HCl(aq) and 0.075 M in HBr(aq) at 25°C.
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the pH for this is the sum of the two concentrations so 0.025 M+ 0.075 M = 0.10 M H then with the
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calculate the pH and the pOH of an aqueous solution that is 0.035 M In HCI and 0.080 M in HBr?
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To calculate the pH and pOH of the aqueous solution, we can use the concentration of HCl and HBr.
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Calculate the Ph and POH of an aqueous soltuion that is 0.500 M in HCl(aq) and 0.085 M in HBr (aq) at 25 degrees C.
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HCl is a strong acid; i.e., it ionizes 100%. Same for HBr. So the combined M in the solution is
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Calcualte PH and POh of an aqueous solution that is 0.050 M in HCL and 0.085 M in HBr at 25 degrees C
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To calculate the pH and pOH of an aqueous solution, you need to know the concentration of the acid
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Complete this table of values for four aqueous solutions at 25 °C.
Solution A: [H+]=0.0093M [OH-]=? pH=? pOH=? Solution B:
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See above.
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Complete this table of values for four aqueous solutions at 25 °C.
Solution A: [H+]=0.0093M [OH-]=? pH=? pOH=? Solution B:
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All of these follow two/three formulas. (H+)(OH^-) = Kw = 1E-14 pH = -log(H^+) pOH = -log(OH^-) pH +
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Each value below represents a different aqueous solution at 25 °C. Classify each solution as acidic, basic, or neutral.
pH=9.72
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you're :)
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