The chemical reaction involved in this titration process would be:
NaOH(aq) + KHC8H4O4(aq) = KNaC8H4O4(aq) + H2<span>O(l)
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To determine the concentration of the NaOH solution, we, first, need to calculate the moles of NaOH that is used up in the reaction given the amount of KHP solution that is used. We do as follows:
Moles NaOH = 0.500 M KHP ( .025 L solution ) ( 1 mol NaOH / 1 mol KHP ) = 0.0125 mol NaOH reacted
Volume of NaOH solution used = 53.5 mL - 25.0 = 28.5 mL
Molarity is the number of moles of a solute per liter of solution. We calculate as follows:
Molarity of NaOH = 0.0125 mol / .0285 mL = 0.44 M
Answer:
It becomes negative
Explanation:
protons carry a positive charge
neutrons carry a neutral charge
electrons carry a negative charge
if we add 2 more electrons, the charge of the ion becomes negative
thank you.
The compound that is a saturated hydrocarbon is CH3CH2OH.
The answer is letter A. A saturated hydrocarbon has only one single bond between the carbon atoms. The compound
that is an unsaturated hydrocarbon is CHCH. The answer is letter D.
This may help you
Allright for <span><span>H2</span>O:</span>
- The central atom is? --> the oxygen atom
- How many atoms are bonded to the central atom? --> 2 hydrogen atoms
- How many lone pairs of electrons are on the central atom? --> O has 6 electrons and has 2 single bonds, so 2 pairs
- How many single bonds are there in this molecule? --> 2
- How many multiple bonds (double and/or triple) are there in this molecule? --> none
For each of your molecules, answer the following questions:
1. Determine the electronegativity between the atoms of each molecule.
Electronegativity O = 3.44
Electronegativity H = 2.20
3.44-2.20=1.24, so the electronegativity between O and H = 1.24
2. Identify the bond as either ionic or covalent.
Electronegativity of 0.0-1.7 = covalent
Electronegativity of 1.7-3.3 = ionic
So it's a covalent bond
3. State whether the molecule is polar or non polar.
Electronegativity of 0.5-1.7= polar covalent
4. Identify the structure as having hydrogen bonding, dipole-dipole moments or London dispersion forces (LDF).
<span><span>H2</span>O</span><span> = hydrogen bonding</span>
<span>The best choice is hypochlorous acid nitrous acid (HNO2) because it has the nearest value of pK to the desired pH.
pKa of </span>nitrous acid<span> is 3.34
If we know pKa and pH values, we can calculate the required ratio of conjugate base (NO2⁻) to acid (HNO2) from the following equation:
pH=pKa + log(conc. of base)/( conc. of acid)
</span><span>3.19=3.34 + log c(NO2⁻)/c(HNO2)
</span><span>3.19 - 3.34 = log c(NO2⁻)/c(HNO2)
-0.15 = log c(NO2⁻)/c(HNO2)
c(NO2⁻)/c(HNO2) = 10⁰¹⁵ = 1.41
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