Answer:
(a) 1:3
(b)
mmol of OH⁻ = 1.893 mmol
mmol of H₃C₆H₅O₇: 0.6310 mmol
mass of H₃C₆H₅O₇: 0.1212 g
mass % of H₃C₆H₅O₇ in orange juice: 1.37%
molarity of H₃C₆H₅O₇ in orange juice: 0.0726 M
Explanation:
Let's consider the following balanced chemical equation.
H₃C₆H₅O₇ + 3 OH⁻ → C₆H₅O₇³⁻ + 3 H₂O
<em>(a) What is the stoichiometry of H₃C₆H₅O₇ to OH⁻? </em>
The molar ratio of H₃C₆H₅O₇ to OH⁻ is 1:3
<em>(b)</em>
<em>mmol of OH⁻: ?</em>

<em>mmol of H₃C₆H₅O₇: ?</em>

<em>mass of H₃C₆H₅O₇: ?</em>
The molar mass of the citric acid is 192.1 g/mol.

<em>mass % of H₃C₆H₅O₇ in orange juice: ?</em>

<em>molarity of H₃C₆H₅O₇ in orange juice: ?</em>

A change in color, odor, or texture
(Also rust)
Answer:
c) yellow precipitate of Agl is formed
Explanation:
KI + AgNO3 = AgI (s)+ KNO3
c) yellow precipitate of Agl is formed
Answer:
Generally, a gas behaves more like an ideal gas at higher temperature and lower pressure, as the potential energy due to intermolecular forces becomes less significant compared with the particles' kinetic energy, and the size of the molecules becomes less significant compared to the empty space between them.
Explanation: