Answer:
The molarity of the acetic acid in this vinegar is 0.853 M
Explanation:
Step 1: Data given
Volume of vinegar sample = 10.00 mL
Concentration of NaOH = 0.5052 M
16.88 mL are required to neutralize the acetic acid
Step 2: The reaction
HC2H3O2(aq) + NaOH(aq) ⇔ NaC2H3O2(aq) + H2O(l)
Step 3: Calculate molarity of cetic acid (HC2H3O2)
C1*V1 = C2*V2
⇒with C1 = the molarity ofHC2H3O2= TO BE DETERMINED
⇒with V1 = the volume of HC2H3O2 = 10.00 mL = 0.01 L
⇒with C2 = the molarity of NaOH = 0.5052 M
⇒with V2 = the volume of NaOH = 16.88 mL = 0.01688L
C1 = (C2*V2)V1
C1 = (0.5052 * 0.01688 ) / 0.01
C1 = 0.853 M
The molarity of the acetic acid in this vinegar is 0.853 M
CO2 is the emperical formula of carbon dioxide
Answer:
the ans
Explanation:
Sodium + chlorine → sodium chloride
The balanced chemical equation:
2Na + Cl2 → 2NaCl
According to the equation above: n(Na) = n(NaCl)
Moles of Na = Mass of Na / Molar mass of Na
The molar mass of Na is 22.9898 g mol-1.
Hence,
n(Na) = 86.33 g / 22.9898 g mol-1 = 3.755 mol
n(NaCl) = n(Na) = 3.755 mol
Moles of NaCl = Mass of NaCl / Molar mass of NaCl
Mass of NaCl = Moles of NaCl × Molar mass of NaCl
The molar mass of NaCl is 58.44 g mol-1.
Hence,
m(NaCl) = 3.755 mol × 58.44 g mol-1 = 219.44 g
m(NaCl) = 219.44 g
OR:
(86.33 g Na)×(1 mol Na/22.9898 g Na)×(2 mol NaCl/2 mol Na)×(58.44 g NaCl/1 mol NaCl) = 219.45 g
Answer: 219.44 grams (or 3.755 mol) of sodium chloride (NaCl) will be produced.
If a substance is reduced, it must undergo a gain of hydrogen or a loss of oxygen.
Reduction
Redox reactions include a change in the oxidation state of the substrate.
Loss of electrons or a rise in an element's oxidation state is considered to be oxidation.
Gaining electrons or lowering the oxidation state of an element or its constituent atoms are both examples of reduction.
Redox reactions fall into one of two categories:
A single electron is transferred from the reducing agent to the oxidant in this process. The terminology used to describe this kind of redox reaction is frequently redox couples and electrode potentials.
A process called atom transfer involves moving an atom from one substrate to another. For instance, as iron rusts, the oxidation state of the iron atoms increases as it transforms into an oxide, while oxygen's oxidation state falls as oxygen receives the electrons released by the iron. Other chemical species can perform the same function, despite the fact that oxidation reactions are frequently linked to the production of oxides. In hydrogenation, hydrogen atoms are transferred in order to weaken C=C bonds.
To learn about the reduction refer here:
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