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3 years ago

The pH of a Ba(OH) 2 solution is 10.00. What is the H+ ion concentration of this solution?

Chemistry

1 answer:

I am Lyosha [343]3 years ago

7 0

Answer:

Option D. 1×10¯¹⁰ M

Explanation:

From the question given above, the following data were obtained:

pH = 10

Hydrogen ion concentration, [H+] =?

The hydrogen ion concentration, [H+] of the Ba(OH)2 solution can be obtained as follow:

pH = – Log [H+]

pH = 10

10 = – Log [H+]

Divide both side by – 1

– 10 = Log [H+]

Take the antilog of – 10

[H+] = antilog (– 10)

[H+] = 1×10¯¹⁰ M

Therefore, the hydrogen ion concentration, [H+] of the Ba(OH)2 solution is 1×10¯¹⁰ M

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If a plant produces 3.21 mol of c6h12o6, how many moles of co2 are needed?

xenn [34]

Photosynthesis is the process by which CO₂ is converted to an organic compound. The complete reaction is as follows;
6CO₂ + 6H₂O --> C₆H₁₂O₆ + 6O₂
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For 1 mol of C₆H₁₂O₆ to be formed - 6 mol of CO₂ is required
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3 0

3 years ago

Consider the substances below.

ratelena [41]

Answer:

They have the same number of atoms. = YES

They have different masses. = YES

Explanation:

1 mol of beryllium

• 1 mol of salt

beryllium = Be = Atomic mass: 9.012182

salt = NaCl = Molar mass: 58.44 g/mol

1 mol of water

• 1 mol of hydrogen

water = H2O = Molar mass: 18.01528 g/mol

hydrogen = H = 1g/mole

Which statement is true about these substances?

They have exactly the same mass. = NO

They have different numbers of particles = NO

They have the same number of atoms. = YES

They have different masses. = YES

Avogadro constant means the number of units in one mole of any substance (defined as its molecular weight in grams) is equal to 6.02214076 × $10^{23}$ .

6 0

3 years ago

Calculate the EMF between copper and silver Ag+e-E=0.89v<br>Cu=E=0.34v

bogdanovich [222]

Answer:

Depending on the $E^\circ$ value of $\rm Ag^{+} + e^{-} \to Ag\; (s)$ , the cell potential would be:

$0.55\; \rm V$ , using data from this particular question; or
approximately $0.46\; \rm V$ , using data from the CRC handbooks.

Explanation:

In this galvanic cell, the following two reactions are going on:

The conversion between $\rm Ag\; (s)$ and $\rm Ag^{+}$ ions, $\rm Ag^{+} + e^{-} \rightleftharpoons Ag\; (s)$ , and
The conversion between $\rm Cu\; (s)$ and $\rm Cu^{2+}$ ions, $\rm Cu^{2+}\; (aq) + 2\, e^{-} \rightleftharpoons \rm Cu\; (s)$ .

Note that the standard reduction potential of $\rm Ag^{+}$ ions to $\rm Ag\; (s)$ is higher than that of $\rm Cu^{2+}$ ions to $\rm Cu\; (s)$ . Alternatively, consider the fact that in the metal activity series, copper is more reactive than silver. Either way, the reaction is this cell will be spontaneous (and will generate a positive EMF) only if $\rm Ag^{+}$ ions are reduced while $\rm Cu\; (s)$ is oxidized.

Therefore:

The reduction reaction at the cathode will be: $\rm Ag^{+} + e^{-} \to Ag\; (s)$ . The standard cell potential of this reaction (according to this question) is $E(\text{cathode}) = 0.89\; \rm V$ . According to the 2012 CRC handbook, that value will be approximately $0.79\; \rm V$ .

The oxidation at the anode will be: $\rm Cu\; (s) \to \rm Cu^{2+} + 2\, e^{-}$ . According to this question, this reaction in the opposite direction ( $\rm Cu^{2+}\; (aq) + 2\, e^{-} \rightleftharpoons \rm Cu\; (s)$ ) has an electrode potential of $0.34\; \rm V$ . When that reaction is inverted, the electrode potential will also be inverted. Therefore, $E(\text{anode}) = -0.34\; \rm V$ .

The cell potential is the sum of the electrode potentials at the cathode and at the anode:

$\begin{aligned}E(\text{cell}) &= E(\text{cathode}) + E(\text{anode}) \\ &= 0.89 \; \rm V + (-0.34\; \rm V) = 0.55\; \rm V\end{aligned}$ .

Using data from the 1985 and 2012 CRC Handbook:

$\begin{aligned}E(\text{cell}) &= E(\text{cathode}) + E(\text{anode}) \\ &\approx 0.7996 \; \rm V + (-0.337\; \rm V) \approx 0.46\; \rm V\end{aligned}$ .

5 0

3 years ago

NH_{4}Cl and NaCl<br> Balanced Equation<br> Total Ionic Equation<br> Net Ionic Equation

nadya68 [22]

Answer:

Based on compounds given, NO reaction occurs

Explanation

The compounds should exchange ions to generate a driving force that pulls the reaction to completion. => Example ...

The Molecular Equation is ...

NH₄Cl(aq) + AgNO₃(aq) => NH₄NO₃(aq) + AgCl(s)

Silver chloride forms in this reaction as a solid precipitate because of its low solubility and is the 'Driving Force' of the reaction. Driving Force is a more stable compound than any on the reactant side and when formed leaves the reaction system as a solid ppt, liquid weak electrolyte (i.e., weak acid or weak base) or a gas decomposition product of a weak electrolyte.

The Ionic Equation is ...

NH₄⁺(aq) + Cl⁻(aq) + Ag⁺(aq) + NO₃⁻(aq) => NH₄⁺(aq) + NO₃⁻(aq) + AgCl(s)

This shows all ions from reaction plus the Driving Force of the reaction.

The Net Ionic Equation is ...

Ag⁺(aq) + Cl⁻(aq) => AgCl(s)

The Net Ionic Equation shows only those ions undergoing reaction. The NH₄⁺ and NO₃⁻ ions are 'Spectator Ions' and do not react.

Attached is a reference sheet for determining the Driving Force of a Metathesis Double Replacement Reaction. Suggest reviewing acid-base theories and the products of decomposition type reactions.

6 0

3 years ago

If the same materials are used to build a voltaic cell and an electrolytic cell, how would the chemical reactions compare?

nadya68 [22]

In the electrolytic cell, depending on the polarity of the battery, either a more vigorous reaction (though the same as the voltaic cell) would occur, or the reverse would.

3 0

3 years ago