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A: Mass of Ba(OH)2 = 407 mg Molar mass of Ba(OH)2 = 171 g/mol Moles = mass/MM = 407/171 = 2.38 mmol…
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- Calculate the pH of the amphiprotic salt NaHA. Ka (H2A) = 0.0026, Ka (HA-) = 0.0000000077pHpH is a logarithmic scale used to indicate the hydrogen ion concentration, [H+], of a solution: pH=−log[H+] Due to the autoionization of water, in any aqueous solution, the hydrogen ion concentration and the hydroxide ion concentration, [OH−], are related to each other by the Kw of water: Kw=[H+][OH−]=1.00×10^−14 where 1.00×10^−14 is the value at approximately 297 K. Based on this relation, the pH and pOH are also related to each other as 14.00=pH+pOH The temperature for each solution is carried out at approximately 297 K where Kw=1.00×10^−14 A. 0.20 g of hydrogen chloride (HCl) is dissolved in water to make 5.5 L of solution. What is the pH of the resulting hydrochloric acid solution? B. 0.20 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 3.0 L of solution. What is the pH of this solution? C. Calculate the concentration of HSO4− ions in a 0.010 M aqueous solution of sulfuric acid.We did an experiment in a lab. We tested for the strength of acids and bases using a conductivity test. Distilled water was used as one of the solutions. the litmus paper and phenolphthalein did not change color. It did not also conduct electricity. Hence it was assumed to be a nonelectrolyte therefore a neutral solution. However, upon searching the internet, it was found that water is not exactly acidic. A pH of 7 at 25°C represents PURE distilled water. Distilled water is considered to be slightly acidic because it absorbed carbon dioxide from the air. The pH of distilled water can range anywhere between 5.5 and 6.9, depending on how long it has been exposed to air. If this is true, then shouldn't the distilled water conduct electricity since acids conduct electricity? Yes or No? please provide an explanation and chemical equation if possible. thank you!
- The base protonation constant K, of lidocaine (C H2 NONH) is 1.15 x 10 . Calculate the pH of a 1.0 M solution of lidocaine at 25 °C. Round your answer to 1 decimal place. pH =A chemist dissolves 773. mg of pure barium hydroxide in enough water to make up 70. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Round your answer to 2 significant decimal places. x10Over the past 250 years, the average upper-ocean pH near the Pacific Northwest has decreased by about 0.1 units, from about 8.2 to 8.1. This drop in pH corresponds to an increase in acidity of about 30%. When CO2 levels in seawater rise, the availability of carbonate ion, CO32−, This makes it more difficult for marine organisms to build and maintain shells and other body parts from calcium carbonate. Calculate H3O+ and OH− concentrations at pH levels of 8.2 and 8.1. Demonstrate by calculations that this decrease in pH corresponds to an increase in acidity of about 30%. Explain the relationship between the pH of seawater and the availability of carbonate ion. Does the change in pH from 8.2 to 8.1 result in an increase or decrease in the availability of carbonate ion?
- Consider the following data on some weak acids and weak bases: acid base 9. name formula name formula HNO, 4.5 x 10 C;H;N |1.7× 10 nitrous acid pyridine hypochlorous acid 8. HСIО |3.0х 10 methylamine CH;NH, |4.4 × 10-4 Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 М KCIO v choose one 1 (lowest) 0.1 M C5H5NHCI 3 0.1 M NaNO2 4 (highest) 3 0.1 М KNO3 choose onePhthalic acid is a diprotic acid with ionization constants Kal = 1.12 × 10−³ and Ka2 = 3.90 × 10-6. Calculate the pH of a 0.237 M potassium hydrogen phthalate (KHP) solution. pH =A chemist dissolves 461. mg of pure barium hydroxide in enough water to make up 180. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Round your answer to 3 significant decimal places. x10
- Over the past 250 years, the average upper-ocean pH near the Pacific Northwest has decreased by about 0.1 units, from about 8.2 to 8.1. This drop in pH corresponds to an increase in acidity of about 30%. When CO2 levels in seawater rise, the availability of carbonate ion, CO32−, makes it more difficult for marine organisms to build and maintain shells and other body parts from calcium carbonate. Calculate H3O+ and OH− concentrations at pH levels of 8.2 and 8.1. Demonstrate by calculations that this decrease in pH corresponds to an increase in acidity of about 30%. Explain the relationship between the pH of seawater and the availability of carbonate ions. Does the change in pH from 8.2 to 8.1 result in an increase or decrease in the availability of carbonate ions?A chemist dissolves 230. mg of pure barium hydroxide in enough water to make up 90. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Be sure your answer has the correct number of significant digits.The base protonation constant K of morpholine (C₂HONH) is 2.14 × 10¯6. Calculate the pH of a 1.0 M solution of morpholine at 25 °C. Round your answer to 1 decimal place. pH = X