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IRISSAK [1]
3 years ago
15

A tablet of one antacid contains citric acid, H3C6H5O7, and sodium hydrogen carbonate, NaHCO3. When the tablet dissolves in wate

r, bubbles of CO2 are produced. This reaction is represented by the incomplete equation below.
H3C6H5O7(aq) + 3NaHCO3(aq)==> Na3C6H5O7(aq) + 3CO2(g) + 3 _______ (ℓ)
Complete the equation in your answer booklet by writing the formula of the missing product.
Chemistry
2 answers:
Nadusha1986 [10]3 years ago
8 0
H2O
This equation is a double displacement reaction, and it forms H2CO3, which is very unstable and separates into H2O and CO2.
scoundrel [369]3 years ago
3 0

Answer:

Water (H₂O) is the missing product

Explanation:

Let's write the equation involved:

H₃C₆H₅O₇(aq) + 3NaHCO₃(aq) ---->

When we watch the first product which is Na₃C₆H₅O₇, we can see that in this case, there was a displacement of the H₃ by the atoms of Na. This give us an idea of what kind of reaction is ocurring. If we follow the principle of the displacement, the reaction should be the following:

H₃C₆H₅O₇(aq) + 3NaHCO₃(aq) ----> Na₃C₆H₅O₇(aq) + 3H₂CO₃(aq)

However, this last compound (H₂CO₃) is very unstable in the presence of sodium citrate, so, the acid suffers another internal reaction:

H₂CO₃(aq) -------> CO₂(g) + H₂O(l)

The CO₂ are the bubbles produced, and the water is produced in solution. Therefore, the products of the general reaction is:

H₃C₆H₅O₇(aq) + 3NaHCO₃(aq) ----> Na₃C₆H₅O₇(aq) + 3CO₂(g) + 3H₂O(l)

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An aqueous basic solution has a concentration of 0. 050 m and kb is 4. 4 × 10^-4. What is the concentration of hydronium ion in
Alex_Xolod [135]

An aqueous basic solution has a concentration of 0. 050 m and kb is 4. 4 × 10^-4, the concentration of hydronium ion in this solution (m) is 2.234 × 10⁻¹² M.

Methylamine is an amine which is an organic weak base. Its chemical formula is CH₃NH₂. When it undergoes hydrolysis wherein water is acting as an acid, the reaction would be

CH₃NH₂ + H₂O ⇆  CH₃NH₃ + OH⁻

Then, we use the ICE analysis which stands for Initial-Change-Equilibrium.

CH₃NH₂ + H₂O ⇆  CH₃NH₃ + OH⁻

Initial                    0.05          -                 0         0

Change                 -x                              +x       +x

----------------------------------------------------------------------------

Equilibrium         0.05-x                           x          x

Then, we use the equation for the equilibrium constant of basicity.

Kb = [CH₃NH₃][OH⁻]/[CH₃NH₂] = 4.4×10⁻⁴

4.4×10⁻⁴ = [x][x]/[0.05-x]

[x] = 4.4756×10⁻³

Here, variable x denotes the number of moles of the substance which is involved in the reaction. Since the equilibrium amount of OH⁻ is equal to x, then the concentration of OH⁻ is also 4.4756×10⁻³. Thus,

pOH = -log[OH⁻]

pOH = -log[4.4756×10⁻³] = 2.35

The relationship between pOH and pH is that pH + pOH = 14. Thus,

pH = 14 - 2.35 = 11.65

pH = -log[H⁺]

11.65 = -log[H⁺]

[H⁺] = 2.234 × 10⁻¹² M

Thus, we find the concentration of solution is 2.234 × 10⁻¹² M.

Learn more about aqueous solution: brainly.com/question/11097800

#SPJ4

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