Concept explainers
Interpretation:
The value of ion-product for water should be determined at
Concept Introduction:
The concentration of hydrogen ions in a solution determines the acidity of a solution. If concentration of hydrogen ion is more than the solution is more acetic, if it is low, solution is less acidic.
The pH of solution is defined as negative log of hydrogen ion concentration thus, it can be calculated as follows:
Here,
Similarly, pOH of a solution is defined as negative log of hydroxide ion concentration thus, it can be calculated as follows:
Here,
pH and pOH of a solution are related to each other as follows:
In a pH scale, if the value of pH is below 7 the solution is said to be acidic in nature, if the pH value is above 7 it is said to be basic in nature. At pH 7, the solution is neutral.
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Chapter 16 Solutions
Introductory Chemistry: A Foundation
- Repeat the description for Question 4, but use a weak acid rather than a strong one.arrow_forwardCommon Acids and Bases Use the data in Table 18.8 to answer the following questions. Which substance is the most basic? Which substance is closest to neutral? Which has a concentration of H+=4.01010M ? Which has a pOH of 11.0? How many times more basic is antacid than blood?arrow_forwardIonization of the first proton from H2SeO4 is complete (H2SeO4 is a strong acid); the acid-ionization constant for the second proton is 1.2 102. a What would be the approximate hydronium-ion concentration in 0.150 M H2SeO4 if ionization of the second proton were ignored? b The ionization of the second proton must be considered for a more exact answer, however. Calculate the hydronium-ion concentration in 0.150 M H2SeO4, accounting for the ionization of both protons.arrow_forward
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- 6. What is a solution with a pOH value of 2 considered? O Salt O Acid Base ONeutralarrow_forwardA student says :- "A solution with [OH^-] = 0.010 M must contain an acid that is stronger than the acid in a solution with [H3O^+] = 0.0050 %3D М." Explain why the student is incorrect. Can you help me with this question, please. It is urgent.arrow_forwardCalculate the concentrations of all species in a 0.940 M Na, SO, (sodium sulfite) solution. The ionization constants for sulfurous acid are Kal = 1.4 × 10-2 and K42 = 6.3 × 10–8. [Na*] = 1.88 [so}] = 0.94 M M [HSO;] = 3.8 x10 -4 1.65 x10-8 M [H,SO,] M Incorrect [OH] = 3.8 x10¬4 [H*] = 2.6 x10-11 M Marrow_forward
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