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
- Ionization of the first proton from H2SO4 is complete (H2SO4 is a strong acid); the acid-ionization constant for the second proton is 1.1 102. a What would be the approximate hydronium-ion concentration in 0.100 M H2SO4 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 0.100 M H2SO4, accounting for the ionization of both protons.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_forwardRepeat the description for Question 4, but use a weak acid rather than a strong one.arrow_forward
- Ionization 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_forwardUsing the acid ionization constant information given in Table 10-3, indicate which acid is the stronger in each of the following acid pairs. a. H3PO4 and H2PO4 b. H3PO4 and H2CO3 c. HPO42 and H2PO4 d. HC2H3O2 and HCNarrow_forwardSuppose a 0.14 M aqueous solution of oxalic acid (H₂C₂O₂) is prepared. Calculate the equilibrium molarity of CO,. You'll find information on the properties. of oxalic acid in the ALEKS Data resource. Round your answer to 2 significant digits. M D.P X Sarrow_forward
- The base protonation constant K, of allantoin (C,H4N3O3NH,) is 9.12 x Calculate the pH of a 1.3 M solution of allantoin at 25 °C. Round your answer to 1 decimal place. 10 6 pH =arrow_forwardFor 6 and 7, use the table of K, values compiled at 25 °C to answer the questions below: Acid HNO3 HCI HBr H2SO4 HSO41 HF HNO2 HCOOH Infinite Infinite Infinite Infinite Ka 1.3 x 102 7.1 x 104 4.5 x 104 1.7 x 104 (Strong acid) HC2041 6.1 x 105 (Strong acid) CH3COOH (Strong acid) (Strong acid) HCO31 4.8 x 1011 Acid C6H5COOH H2CO3 H2PO41 HCN НРОД? Ka 6.5 x 105 1.8 x 106 4.2 x 107 6.2 x 108 4.9 x 1010 4.8 x 1013 6. Which of the following has the highest pH? a. 1.00 M NaNO3 b. 1.00 M NaNO2 с. 1.00 М NaH2РОд d. All have the same pH 7. Which of the following has the lowest pH in aqueous solution? a. 1.00 M NaCl b. 1.00 M NaNO3 c. 1.00 M NaBr d. All have the same pHarrow_forward6. What is a solution with a pOH value of 2 considered? O Salt O Acid Base ONeutralarrow_forward
- The pH of blood is 7.4. What is the ratio (to one decimal place) of bicarbonate (conjugate base) to carbonic acid (weak acid) in the blood's buffering equilibrium? Note, the K₂ of carbonic acid is 4.27 x 10-7. Write your answer this way: # to 1 Done Clear Incorrect. The ratio is 10.7 to 1, indicating that there is 10 times more bicarbonate than carbonic acid. Enter the correct answer.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_forwardCalculate the [H† of a solution at 25 °C that has a p)H = 5.43. Type your answer...arrow_forward
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