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The ionic product of water is defined as (1) The product of the concentration of proton and hydroxyl ion in pure water (2) The product of the concentration of acid and hydroxyl ion in aqueous solution (3) The ratio of the concentration of dissociated water to the undissociated water (4) All the above

Short Answer

Expert verified
Option (1) is correct.

Step by step solution

01

Define Ionic Product of Water

The ionic product of water, commonly denoted as \(K_w\), is defined for pure water as the product of the concentrations of the hydrogen ion (proton) \([H^+]\) and the hydroxyl ion \([OH^-]\).
02

Explore Given Options

Analyze each given option to check which one correctly corresponds to the definition of the ionic product of water.
03

Verify Option (1)

Option (1): 'The product of the concentration of proton and hydroxyl ion in pure water' matches the definition of the ionic product of water, \([H^+][OH^-]\).
04

Verify Option (2)

Option (2) talks about the product of the concentration of acid and hydroxyl ion in an aqueous solution. This doesn't correspond directly to the definition of \(K_w\).
05

Verify Option (3)

Option (3) mentions the ratio of the concentration of dissociated water to undissociated water, which is not the same as the ionic product of water.
06

Verify Option (4)

Option (4) claims that all the given statements are correct. Since not all options correspond to the definition of the ionic product of water, this option is incorrect.
07

Conclusion

Based on the evaluation, the correct option is (1), which accurately describes the ionic product of water.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Proton Concentration
In chemistry, the term 'proton concentration' refers to the concentration of hydrogen ions, often denoted as \([H^+]\). Protons are positively charged atoms that are released when an acid dissociates in water. In pure water, the concentration of protons is extremely low because water is only very slightly ionized. This proton concentration is one of the two critical components when we talk about the ionic product of water, \([K_w]\). The formula representing proton concentration in water is:
\([H_2O] \leftrightharpoons H^+ + OH^-\)
Here, \([H^+]\) is the proton concentration.

To measure acid or base strength, we look at the \([H^+]\) concentration.
  • Strong acids have high \([H^+]\) concentrations.
  • Weak acids have relatively low \([H^+]\) concentrations.
Knowing \([H^+]\) is crucial to understanding the reactivity and characteristics of substances in aqueous solutions.
Hydroxyl Ion Concentration
Hydroxyl ion concentration refers to the concentration of \([OH^-]\) ions in a solution. Hydroxyl ions are negatively charged and typically arise from the dissociation of bases. In the context of water's autoionization, the equation is:
\([H_2O] \leftrightharpoons H^+ + OH^-\)
This shows that water dissociates into equal parts hydrogen ions and hydroxyl ions. The concentration of hydroxyl ions in pure water is quite low but equal to that of hydrogen ions, both being \[10^{-7}\] M at 25°C.

  • Strong bases have high \([OH^-]\) concentrations.
  • Weak bases have relatively lower \([OH^-]\) concentrations.
Understanding \([OH^-]\) concentration is essential when analyzing pH and pOH, as these values can tell us how acidic or basic a solution is.
Kw Constant
The ionic product of water, denoted as \[K_w\], is a critical concept. For pure water at 25°C, \[K_w\] is expressed as:
\[K_w = [H^+][OH^-]\]
The value of \([K_w]\) is \[1 \times 10^{-14} M^2\]. This means that the product of the concentrations of hydrogen ions and hydroxyl ions in pure water is constant at this temperature.

If we increase the temperature, the value of \([K_w]\) also increases, and vice versa. This constant forms the foundation for understanding the pH scale, where:
  • pH = -log\([H^+]\)
  • pOH = -log\([OH^-]\)
Additionally, in any aqueous solution, the product of \([H^+]\) and \([OH^-]\) must equal \([K_w]\). This constraint helps chemists predict and manipulate the acidity and basicity of solutions by adjusting ion concentrations.

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Most popular questions from this chapter

Sodium carbonate cannot be used in place of ammonium carbonate for the identification of the fifth group radicals. This is because the (1) sodium ions will interfere in the detection of the fifth group radicals (2) concentration of carbonate ions is very low (3) sodium will react with acidic radicals (4) magnesium will be precipitated

For the reaction \(\mathrm{Ag}_{2} \mathrm{CO}_{3}(\mathrm{~s}) \rightleftharpoons \mathrm{Ag}_{2} \mathrm{O}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g})\) the value of the equilibrium constant \(\mathrm{K}_{\mathrm{p}}\) is \(3.16 \times 10^{3}\) atm at \(298 \mathrm{~K}\) and is \(1.48 \mathrm{~atm}\) at \(500 \mathrm{~K}\); then which one of the following statements is correct? (1) The yield of \(\mathrm{CO}_{2}\) is independent of temperature. (2) The yield of \(\mathrm{CO}_{2}\) will increase at high pressure. (3) The value of \(\Delta H\) for the forward reaction is negligible. (4) The forward reaction is endothermic.

According to Bronsted Lowry concept the correct order of strength of bases follows the order (1) \(\mathrm{CH}_{3} \mathrm{COO}^{-}>\mathrm{OH}^{-}>\mathrm{Cl}^{-}\) (2) \(\mathrm{OH}^{-}>\mathrm{CH}_{3} \mathrm{COO}^{-}>\mathrm{Cl}^{-}\) (3) \(\mathrm{CH}_{3} \mathrm{COO}^{-}>\mathrm{Cl}^{-}>\mathrm{OH}^{-}\) (4) \(\mathrm{OH}^{-}>\mathrm{Cl}^{-}>\mathrm{CH}_{3} \mathrm{COO}^{-}\)

When \(\mathrm{NaCl}\) is added to the reaction mixture of an oil and caustic soda, the soap is thrown out because (1) \(\mathrm{NaCl}\) is an ionic compound (2) Soap is insoluble in the presence of chloride ions (3) The solubility product of \(\mathrm{NaCl}\) decreases in the presence of soap (4) The solubility product of the soap is excceded duc to the increased concentration of \(\mathrm{Na}^{-}\) ions

Which of the following statements is false? (l) According to Lewis theory electrophiles are Lewis acids while nucleophiles are Lewis bases. (2) In Friedel-Crafts reaction, the catalysts used are Lewis acids. (3) In complex compounds, metal ions are Lewis bases while ligands are Lewis acids. (4) Electron-deficient molecules are Lewis acids.

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