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Serga [27]
3 years ago
13

How many milligrams are equal to 0.0265 pounds?

Chemistry
1 answer:
daser333 [38]3 years ago
8 0

Answer:

37.73 pounds

Explanation:

just trust me.

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A solution has a pH of 4.20. Using the relationship between pH and pOH, what is the concentration of OH−?
frez [133]

Answer : The concentration of OH^- ion is, 1.58\times 10^{-10}M

Solution : Given,

pH = 4.20

First we have to calculate the pOH.

As we know that,

pH+pOH=14

pOH=14-pH

pOH=14-4.20

pOH=9.8

Now we have to calculate the concentration of OH^- ion.

pOH=-\log [OH^-]

9.8=-\log [OH^-]

[OH^-]=1.58\times 10^{-10}M

Therefore, the concentration of OH^- ion is, 1.58\times 10^{-10}M

4 0
3 years ago
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The mass number of an atom is determined by ___.
Ronch [10]

Answer:

2

Explanation:

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3 years ago
Balance the redox reaction Al(s) + MnO4^- (aq) --> MnO2 (s) + Al(OH)4^- (aq) in aqueous basic solution
GREYUIT [131]

Answer:

Al + MnO4- + 2H2O → Al(OH)4- + MnO2

Explanation:

First of all, we out down the skeleton equation;

Al + MnO4- → MnO2 + Al(OH)4-

Secondly, we write the oxidation and reduction equation in basic medium;

Oxidation half equation:Al + 4H2O + 4OH- → Al(OH)4- + 4H2O + 3e-

Reduction half equation:MnO4- + 4H2O + 3e- → MnO2 + 2H2O + 4OH-

Thirdly, we add the two half reactions together to obtain:

Al + MnO4- + 8H2O + 4OH- + 3e- → Al(OH)4- + MnO2 + 6H2O + 3e- + 4OH-

Lastly, cancel out species that occur on both sides of the reaction equation;

Al + MnO4- + 8H2O→ Al(OH)4- + MnO2 + 6H2O

The simplified equation now becomes;

Al + MnO4- + 2H2O → Al(OH)4- + MnO2

4 0
3 years ago
Last one i think.......
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Answer is c i believe
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What is the molar mass of magnesium
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