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kondor19780726 [428]
3 years ago
11

Using the measurements in the table, determine which unidentified metal has the lowest density

Chemistry
2 answers:
Oliga [24]3 years ago
3 0
C is the correct answer because density is mass per unit volume and when you divide it we that volume is greater than mass so density is less density density is directly proportional to Mass Density is inversely proportional to volume
xxTIMURxx [149]3 years ago
3 0

Answer:

\boxed{\text{Metal c}} }

Explanation:

\text{Density} = \dfrac{\text{mass}}{\text{volume}}\\\\\textbf{a. }\text{Density} = \dfrac{\text{122 g}}{\text{12.5 cm}^{3}} = \text{9.96 g/cm}}^{3}\\\\\textbf{b. }\text{Density} = \dfrac{\text{132 g}}{\text{14.2 cm}^{3}}= \text{9.30 g/cm}}^{3}\\\\\textbf{c. }\text{Density} = \dfrac{\text{126 g}}{\text{18.1 cm}^{3}}= \text{6.96 g/cm}}^{3}\\\\\textbf{d. }\text{Density} = \dfrac{\text{126 g}}{\text{12.7 cm}^{3}}= \text{9.92 g/cm}^{3}\\\\\boxed{\textbf{Metal c}}\text{ has the lowest density}

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Read 2 more answers
A buffer solution contains 0.479 M NaHCO3 and 0.342 M Na2CO3. Determine the pH change when 0.091 mol HNO3 is added to 1.00 L of
pshichka [43]

Answer:

ΔpH = 0.20

Explanation:

The buffer of HCO₃⁻ + CO₃²⁻ has a pka of 10.2

HCO₃⁻ ⇄ H⁺ + CO₃²⁻

There are 0.479moles of NaHCO₃ and 0.342moles of Na₂CO₃.

Using Henderson-Hasselbalch formula:

pH = pka + log [Base] / [Acid]

pH = 10.2 + log 0.342mol / 0.479mol

<em>pH = 10.05</em>

NaOH reacts with HCO₃⁻ producing CO₃²⁻, thus:

NaOH + HCO₃⁻ → CO₃²⁻ + H₂O + Na⁺

0.091 moles of NaOH produce the same moles of CO₃²⁻ and consume HCO₃⁻. Moles of these species are:

CO₃²⁻: 0.342mol + 0.091mol: 0.433mol

HCO₃⁻: 0.479mol - 0.091 mol: 0.388mol

Using Henderson-Hasselbalch formula:

pH = pka + log [Base] / [Acid]

pH = 10.2 + log 0.433mol / 0.388mol

pH = 10.25

That means change of pH, ΔpH is:

ΔpH = 10.25 - 10.05 = <em>0.20</em>

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I hope it helps!

3 0
3 years ago
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