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- 8. 200 mL of 0.7M LİOH is titrated with 1.0 M CH,COOH. Ka of acetic acid is 1.8 x 10 i. find the final pH of the solution at equivalence point. (ANS: 8.99) ii. The titration process was stopped at equivalence point. 200 mL of 0.5M CH,COOH was further added into the mix. Please calculate the new pH. (ANS: 4.9)Dissolved carbon dioxide in seawater occurs mainly in three inorganic forms (see figure below): free aqueous carbon dioxide (CO2(aq)), bicarbonate (HCO3), and carbonate ions (CO3²). (a) Using the figure, rank the concentrations of these species from highest to lowest. (b) If surface ocean pH were to fall from 8.0 to 7.0, how would this ranking change? -1.5 2 H+ Surface Ocean pH OH HCO3 -2.5 -3 CO₂ Log [concentration (mol kg¹)] сл + -4.5 50 2 4 6 PH 8 10 co 123 12 146..please help me with both if you can, will rate you up! need this done by the morning.
- (8): Calculate the pH and percent protonation of 0.10 M ammonia NH3 (aq)(use Table 15.9 to find the Kb of this weak base)If the pH of a 0.0850 M solution of HBRO2 is 2.29, then what is the value for the acidity constant, Ką, of HB1O2? HB1O2(aq) + H20(1) H3O*(aq) + BrO2 (aq) K = ? K, for HBrO2: Given the information above, is the bromite ion, BrO2 , a strong base, a weak base, or not basic in water?Phosphorous acid, H,PO, (aq), is a diprotic oxyacid that is an important compound in industry and agriculture. pKal pKa2 но- -P -O- 1.30 6.70 Calculate the pH for each of the points in the titration of H. 50.0 mL of 2.4 M H, PO, (aq) with 2.4 M KOH(aq). before addition of any КОН: after addition of 25.0 mL KOH: after addition of 50.0 mL KOH: after addition of 75.0 mL KOH: after addition of 100.0 mL KOH:
- Weak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/A13.1) a) What is the pH of a 3.6×10-2 M solution of KOH at 25 °C? b) What is the pH of a 3.48×10-2 M solution of the strong acid HClO4? HClO4(aq) + H2O(ℓ) → ClO4-(aq) + H3O+(aq)[HClO4]0 = 3.48×10-29 (a) A and B are white powders. A is insoluble in water but B is soluble in water and its solution has a pH value of 3. A mixture of A and B bubbles or fizzes in water. A gas is given off and a clear solution forms. (1) Which powder is acidic? (ii) The other powder is a carbonate. What gas is given off in the reaction? [1] [1] E (b) Anyhdrous copper(II) sulphate is a white powder. (C) Write its formula. [1] (ii) What happens when water is added to anhydrous copper(II) sulphate [1] (c) Describe two tests to show that a given liquid is water 1 [2]
- the pH of modern rain water (= 5.61) in equilibrium with air at 25°C and a total pressure of 1 atmosphere, with a partial pressure of CO2 (PCO2) = 10-3.4 atmospheres (which equals 400 ppm by volume). The Intergovernmental Panel on Climate Change (IPCC) estimates that CO2 concentrations in 2050 may reach 600 ppm (PCO2 = 10–3.22 atmospheres). (a) Calculate the pH of rain water in equilibrium with 600 ppm of CO2. (b) By what factor (i.e. multiplier) is (H+) higher or lower in 2050 rain water vs. modern rain water? Please answer very soon will give rating surely All questions answers neededOur stomachs contain a solution of roughly 0.03 M HCl, which helps us digest the food we eat. The burning sensation associated with heartburn is a result of the acid of the stomach leaking through the muscular valve at the top of the stomach into the lower reaches of the esophagus. The lining of the esophagus is not protected from the corrosive effects of stomach acid the way the lining of the stomach is, and the results can be very painful. When we have heartburn, it feels better if we reduce the excess acid in the esophagus by taking an antacid. As you may have guessed, antacids are bases. One of the most common antacids is calcium carbonate, CaCO3. Read 7.2. Classifying Chemical Reactions, Acid-Base Reactions, and write the chemistry reaction between HCl and CaCO3Assuming only the neutral form of the compound significantly "bioconcentrates" in fish, Estimate the equilibrium concentration (ug chemical/kg wet fish) of the acid pentachlorophenol (PCP) in a rainbow trout swimming in water (pH =7) having a total concentration of 10 ug/L PCP (both neutral and negatively charged forms. The log Kow for the neutral form of pentachlorophenol is 5.0 and the pKa is 5.
