The concentration in ppm is 0.06 ppm
<h3>How to convert to PPM?</h3>
There are several unit of concentration in chemistry. Let us recall that concentration is the amount of substance that is present in a solution. Thus we have;
Concentration = 9.65 x 10-7 M
Molar mass of potassium cyanide = 65 g/mol
Thus;
M = ppm/MM * 1000
M = molar concentration
MM = molar mass
M * MM * 1000 = ppm
ppm = 9.65 x 10-7 M * 65 g/mol * 1000
ppm = 0.06 ppm
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The question is incomplete. The complete question is:
The half-life for the decay of carbon-14 is 5.73x10^3 years. Suppose the activity due to the radioactive decay of the carbon-14 in a tiny sample of an artifact made of woodfrom an archeological dig is measured to be 2.8x10^3 Bq. The activity in a similiar-sized sample of fresh wood is measured to be 3.0x10^3 Bq. Calculate the age of the artifact. Round your answer to 2 significant digits.
Answer:
570 years
Explanation:
The activity of the fresh sample is taken as the initial activity of the wood sample while the activity measured at a time t is the present activity of the wood artifact. The time taken for the wood to attain its current activity can be calculated from the formula shown in the image attached. The activity at a time t must always be less than the activity of a fresh wood sample. Detailed solution is found in the image attached.
Answer:
Allele
Explanation:
An allele is a variant form of a gene.some gene have a variety of different forms which are located at the same position or gentic locuson a chromosone. human are called diploid organisms becuase they jave two alleles at a each genitic locus with one allele inherited from each parent.
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Answer:
0.200M H₃PO₄
0.600N H₃PO₄
pH = 1.46
Explanation:
The acid-base reaction of phosphoric acid (H₃PO₄) with LiOH is:
3 LiOH + H₃PO₄ → Li₃PO₄ + 3H₂O
<em>Where 3 moles of LiOH reacts per mole of H₃PO₄</em>
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Moles of LiOH are:
0.030L× (0.5mol / L) = 0.0150 moles of LiOH
Moles of acid neutralized are:
0.0150 moles of LiOH × (1 mole H₃PO₄ / 3 moles LiOH) = 0.005 moles H₃PO₄
As volume of acid was 25mL, molarity is:
0.005mol H₃PO₄ / 0.025L =<em> 0.200M H₃PO₄</em>
Normality is:
0.200M × (3N H⁺ / 1M H₃PO₄) = <em>0.600N H₃PO₄</em>
H₃PO₄ dissolves in water thus:
H₃PO₄ ⇄ H₂PO₄⁻ + H⁺
Ka = 7.1x10⁻³ = [H₂PO₄⁻] [H⁺] / [H₃PO₄]
Where molar concentrations in equilibrium will be:
[H₂PO₄⁻] = X
[H⁺] = X
[H₃PO₄] = 0.200M - X
Replacing in Ka formula:
7.1x10⁻³ = [X] [X] / [0.200 - X]
1.42x10⁻³ - 7.1x10⁻³X = X²
0 = X² + 7.1x10⁻³X - 1.42x10⁻³
Solving for X:
X = -0.04M →False answer, there is no negative concentrations.
X = 0.0343M
As, [H⁺] = 0.0343M
pH = - log [H⁺],
<em>pH = 1.46</em>
