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Explain the difference in pH between diH2O and tap water
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- Apatite, Ca5(PO4)3OH, is the mineral in teeth. On a chemical basis explain why drinking milk strengthens young children’s teeth. Sour milk contains lactic acid. Not removing sour milk from the teeth of young children can lead to tooth decay. Use chemical principles to explain why.The active ingredient of bleach such as Clorox is sodium hypochlorite (NaClO). Its conjugate acid, hypochlorous acid (HClO), has a Ka of 3.0 × 10–8. (a)The undiluted bleach contains roughly 1 M NaClO. Calculate the pH of 1 M NaClO solution. (b)Some applications require extremely diluted bleach solution, such as swimming pools. Suppose the solution in (a) is diluted by 10,000 -fold. Calculate the pH of the diluted solution, and demonstrate that you can still neglect the autoionization of water in your calculation. (c)Suppose the solution in (a) is diluted by 1million-fold, briefly explain how your approach will be different. Write the equation with [H3O+] as the unknown, but you do not need to solve it.The active ingredient of bleach such as Clorox is sodium hypochlorite (NaClO). Its conjugate acid, hypochlorous acid (HClO), has a Ka of 3.0 × 10–8. (a) The undiluted bleach contains roughly 1 M NaClO.Calculate the pH of 1 M NaClO solution. (b) Some applications require extremely diluted bleach solution, such as swimming pools. Suppose the solution in (a) is diluted by 10,000-fold. Calculate the pH of the diluted solution, and demonstrate that you can still neglect the autoionization of water in your calculation. (c) Suppose the solution in (a) is diluted by 1 million-fold, briefly explain how your approach willbe different. Write the equation with [H3O+] as the unknown, but you do not need to solve it.
- Calculate the pH of the solution in which 0.2M NH4Cl and 0.1M NH3 are present. The pKb of ammonia solution is 4.75.The active ingredient of bleach such as Clorox is sodium hypochlorite (NaClO). Its conjugate acid, hypochlorous acid (HClO), has a Ka of 3.0 × 10^–8. (a) The undiluted bleach contains roughly 1 M NaClO. Calculate the pH of 1 M NaClO solution. (b) Some applications require extremely diluted bleach solution, such as swimming pools. Suppose the solution in (a) is diluted by 10,000 -fold. Calculate the pH of the diluted solution, and demonstrate that you can still neglect the autoionization of water in your calculation. (c) Suppose the solution in (a) is diluted by 1 million-fold, briefly explain how your approach will be different. Write the equation with [H3O+] as the unknown, but you do not need to solve it.Calculate the pH of a blood plasma sample with a total CO₂ concentration of 25.6 mM and bicarbonate concentration of 24.5 mM. The relevant pKa of carbonic acid is 6.1. Enter the answer with three significant figures. pH = Hyperventilating can result in a decrease in CO₂(g) concentration in the blood. How would this affect the pH of the extracellular fluid? The pH does not change appreciably. The pH increases. The pH decreases.
- Calculate the pH of a sample of rainwater if it is left to cquilibrate with 2.0 ppmv of SO2 (KH = 1.2 molL atm). Assume SO2 is the only acidic gas present. Given: KH (SO2)= 1.2 mol L K (H2SO) = .7 x 10 mol K (H2SO) =6.6 x 10 mol atma) Calculate the pH of an aqueous solution of the salt NaA, which was made to a concentration of 0.080 M NaA. The Ka of the weak acid HA is 2.0 x 10-5. Your pH should go to two places past the decimal point (i.e. 1.35). b) Aniline, C6H5NH2, has a pKb of 9.40. What is the pH of a solution which is 0.12 M in aniline and 0.38 M in anilinium ion, C6H5NH3+? Your answer should be to two places past the decimal.Calculate the degree of ionization of morphine, pKa 8.0, in a solution with a pH of 2.2. Predict how the degree of ionization could affect the ease of absorption of morphine in (a) the stomach and (b) the intestine when the pH of the stomach fluid is 2.0 and the pH of the intestinal fluid is 6.
- 4a) Write an equation for the neutralization reaction of sodium acetate in solution upon addition of HCl.Calculate the pH and pOH of the following solutions (see Appendix 11 of your textbook for pKa values): 1. 0.01 M HBr 2. 0.00005 M HBr 3. 0.00002 МКОН 4. 0.01 M CH,COOH 5. 0.00001 M CH,COOH 6. 0.01 M HIO, 7. 0.01 M pyridine Calculate the pH of the following solutions: 1. 0.01 M NAHS 2. 0.005 M NaН.РО, 3. 0.005 M Na,HPO, 4. 0.005 M Na PO, 5. 0.1 ΜΝΗ,CN Calculate the pH of the following buffer solutions: 1. 1.7 g/L of NH, and 5.35 g/L of NH,Cl. 2. 50 mL of 1 M CH,COONA and 1 L 0.1 M CH,COOH. 3. 50 mL of 1 M NaOH and 1 L 0.1 M CH,COOH. 4. 10 mL 0.1 H,PO, + 25 mL 0.1 NaOH 5. 10 mL 0.1 H,PO, + 25 mL 0.1 Na,PO, 6. A buffer solution pH=5.00 contains 0.01 M CH,COOH. Calculate the concentration of sodium acetate it contains. 7. What weight of NH,Cl should be added to 1 L of 0.1 M NH, solution to get pH=9.00?Calculate the theoretical pH of the solution please 0.100 M aluminum nitrate Hydrated aluminum ion – Al(H2O)63+: pKa = 4.82
