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densk [106]
3 years ago
14

0.17 M KCHO2 Find the pH

Chemistry
1 answer:
SashulF [63]3 years ago
6 0
I believe the pH is 7. If you would like me to explain comment.
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How does the law of definite proportions apply to hydrates?
vladimir1956 [14]
The law of definite proportions would state that a hydrate always contain exactly the same proportion of salt and water by mass.
strictly speaking, the law of definite proportion states that a compound always 
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But the law is often applied to groupings of elements in compound.
Hydrates are salt that have a certain amount of  water asa part of their structure.
The water is chemically combined with the compound in a definite ratio.
4 0
2 years ago
The atomic mass can be smaller than the atomic number
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8 0
3 years ago
Could someone help?
Aleks [24]

Answer:

Mass

Explanation:

I majored on Chemistry

7 0
2 years ago
Read 2 more answers
At a particular temperature a 2.00-L flask at equilibrium contains 2.80 ✕ 10-4 mol N2, 2.50 ✕ 10-5 mol O2, and 2.00 ✕ 10-2 mol N
zhenek [66]

Answer : The value of equilibrium constant (K) is, 5.71\times 10^4

Explanation :

First we have to calculate the concentration of N_2,O_2\text{ and }N_2O

\text{Concentration of }N_2=\frac{\text{Moles of }N_2}{\text{Volume of solution}}=\frac{2.80\times 10^{-4}mol}{2.00L}=1.4\times 10^{-4}M

and,

\text{Concentration of }O_2=\frac{\text{Moles of }O_2}{\text{Volume of solution}}=\frac{2.50\times 10^{-5}mol}{2.00L}=1.25\times 10^{-5}M

and,

\text{Concentration of }N_2O=\frac{\text{Moles of }N_2O}{\text{Volume of solution}}=\frac{2.00\times 10^{-2}mol}{2.00L}=1.00\times 10^{-2}M

Now we have to calculate the value of equilibrium constant (K).

The given chemical reaction is:

N_2(g)+O_2(g)\rightarrow 2N_2O(g)

The expression for equilibrium constant is:

K=\frac{[N_2O]^2}{[N_2][O_2]}

Now put all the given values in this expression, we get:

K=\frac{(1.00\times 10^{-2})^2}{(1.4\times 10^{-4})\times (1.25\times 10^{-5})}

K=5.71\times 10^4

Thus, the value of equilibrium constant (K) is, 5.71\times 10^4

7 0
3 years ago
Hydrobromic acid is added to a solution of lead(II) nitrate. Predict the products, and write a balanced equation for this reacti
Ber [7]

Answer:

2HBr + Pb(NO₃)₂ → PbBr₂ + 2HNO₃

Explanation:

Hydrobromic acid (HBr), reacts with lead (II) nitrate (Pb(NO₃)₂) producing Lead(II) bromide (PbBr₂) and nitric acid (HNO₃). The reaction is:

HBr + Pb(NO₃)₂ → PbBr₂ + HNO₃

This reaction is unbalanced. You can see in products 2 Bromides but in reactants just 1. And in reactants 2 NO₃ but as product just 1. Thus, you can balance the equation, thus:

<em>2HBr + Pb(NO₃)₂ → PbBr₂ + 2HNO₃</em>

And this equation is the answer of your question!

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7 0
3 years ago
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