Answer:If we have [H+][OH-]= Kw = 1.0 x 10^-14
Then [H+]= Kw/ [OH-]= 1.0x 10^-14/ 1 x 10^-11 =1 x 10^-3 mol/L
And here is the solution - as you can see it is an acidic one :
pH = - log [H+]= - log 1 x 10^-3 = 3 < 7
Explanation:
The answer is dissolved in water, because in chemistry, (aq) is shorthand for aqueous solution.
<h2>Ionic bonds result from transferring of electrons</h2>
Explanation:
- Ionic bonds result from transferring of electrons.
- An ionic bond is also referred to as an electrovalent bond.
- The main reason for the formation of the bond is an electrostatic attraction between oppositely charged ions that are cation and anion in a chemical compound.
- The formation of such bonds occurs when the valence (outermost) electrons of one atom are transferred to another atom or the loss of electrons from one atom and gain of electrons of another atom.
- The atom that loses the electrons forms cation that is a positively charged ion.
- The atom that gains electrons forms an anion that is a negatively charged ion.
1 ounces ----------- 29.5735 mL
5 ounces ----------- ??
5 x 29.5735 / 1 => 147.868 mL
hope this helps!
Answer:
2.30 liters.
Explanation:
- The balanced equation of the reaction is:
<em>Na₂O₂ + CO₂ → Na₂CO₃ + 1/2O₂,</em>
- It is clear that 1.0 mole of Na₂O₂ reacts with 1.0 mole of CO₂ to produce 1.0 mole of Na₂CO₃ and 0.5 mole of O₂.
- The no. of moles of CO₂ in (4.60 L) reacted can be calculated from the relation: <em>PV = nRT</em>.
P is the pressure of the gas (P = 1.0 atm at STP),
V is the volume of the gas (V = 4.60 L),
R is the general gas constant (R = 0.082 L.atm/mol.K),
T is the temperature of the gas (T = 273.0 K at STP).
∴ n = PV/RT = (1.0 atm)(4.6 L) / (0.082 L.atm/mol.K)(273.0 K) = 0.205 mol.
<u><em>Using cross multiplication:</em></u>
1.0 mole of CO₂ produces → 0.5 mole of O₂, from the stichiometry.
0.205 mole of CO₂ produces → ??? mole of O₂.
- The no. of moles of O₂ produced from 4.60 L of CO₂ = (0.5 mole)(0.205 mole) / (1.0 mole) = 0.103 mole.
- ∴ The volume of O₂ produced from 4.60 L of CO₂ = nRT/P = (0.103 mol)(0.082 L.atm/mol.K)(273.0 K) / (1.0 atm) = 2.30 liters.
