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marin [14]
3 years ago
8

Calculate the ph of a solution in which [oh–] = 4.5 × 10–9m.

Chemistry
1 answer:
frosja888 [35]3 years ago
5 0

pOH = -LOG([OH])  

pOH = -LOG(4.5*10^-9)  

pOH = 8.34  

pH + pOH = 14  

pH = 14 - 8.34 = 5.65

hope this helps!

(:

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Explanation:

1. Please provide the enthalpy info - I will work on it with the info

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Two solutions are combined in a beaker. One solution contains 500.0 g of potassium phosphate and the other contains 500.0 g of c
Anna [14]

The question is incomplete. The complete question is

Two solutions are combined in a beaker. One solution contains 500.0 g of potassium phosphate and the other contains 500.0 g of calcium nitrate. A double displacement reaction occurs. What mass of each of the following substances is present when the reaction stops. A) potassium phosphate remaining B) calcium nitrate g remaining C) calcium phosphate formed D) potassium nitrate g formed

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Explanation:

The equation of the reaction:

2K3PO4(aq) + 3Ca(NO3)2 (aq)-------> 6KNO3(aq) + Ca3(PO4)2(s)

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b) Amount of calcium nitrate reacted according to reaction equation=3

Amount of calcium nitrate remaining=3.05-3= 0.05

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c) since calcium nitrate is the limiting reactant, we use to estimate the mass of products formed.

From the reaction equation,

3 moles of calcium nitrate yields 1 mole of calcium phosphate

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