As mentioned during the lecture, a higher atmospheric concentration of carbon dioxide leads to lower pH level of rain water. One of the higher-end projections for 2100 forecasts a carbon dioxide concentration of 910 ppm. Calculate the pH of the rainwater for this scenario. Refer to slide 20 of the PowerPoint for help with the calculation.
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- Consider the following data on some weak acids and weak bases: name K₂ formula HNO₂ 4.5 x 104 acetic acid HCH,CO₂ 1.8x105 acid nitrous acid solution 0.1 M HONHYBT 0.1 M KBr 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. 0.1 M KCH₂CO₂ 0.1 M C₂H₂NHCI PH choose one choose one choose one base choose one K name formula hydroxylamine HONH₂ 1.1 x 107 pyridine CH₂N 1.7×102. Aspirin is absorbed into the blood through the cells lining the stomach and the small intestine. Absorption requires passage through the plasma membrane, the rate of which is determined by the polarity of the molecule: charged and extremely polar molecules pass slowly, whereas neutral and hydrophobic ones pass rapidly a. The pH inside the stomach is around 2.0 and the pH of the contents of the small intestine is about 6.0. Which of the following statements is correct: i. The small intestine has 3 times lower [H] than the stomach. ii. The small intestine has 4 times lower [H ] than the stomach iii. The small intestine has 3,000 times lower [H] than the stomach iv. The small intestine has 10,000 times lower [H] than the stomach. b. The pKa of aspirin is 3.5. Draw the predominant form of aspirin and its overall charge (-1,0 or +1) when it is in the stomach or in the small intestine: Small Intestine (pH= 6.0): Stomach (pH 2.0) Overall Charge: Overall Charge:The first step in purifying the urine collected on the ISS is to treat every liter of urine with 20 mL of 1.0 M H2SO4. To simplify the calculations, lets assume that urine is water. a) What is the pH of a solution of 20. mL of 1.0 M H2SO4 added to 1.00 L water? To determine this, you can safely assume that 100% of the H2SO4 reacts to form H3O+ and HSO4- ions. Use pKa2 (1.92) to determine if any more protons are added to the solution from HSO4-.
- Calculate the pH of a raindrop in equilibrium with 8.10 x 10^-8 atm SO2 in the air. Assume no further oxidation of H2SO3. KH for SO2 is 1.2 M/atm Ka for H2SO3 is 0.015 round to 2 decimal pointsWhat is the partial pressure of carbon dioxide in a container that holds 5 moles of carbon dioxide, 3 moles of nitrogen, and 1 mole of hydrogen and has a total pressure of 1.05atm? Show the complete solution. a. PCO2 = 1.588atm; PN = 1.347atm; PH = 1.116atm b. PCO2 = 0.588atm; PN = 0.347atm; PH = 0.116atm c. PCO2 = 2.588atm; PN = 2.347atm; PH = 2.116atm d. PCO2 = 3.588atm; PN = 3.347atm; PH = 3.116atmcom/courses/22672/quiz2es/68142/laRU e G My Policy Details O Strongnet l-Notes... P PowerSchool P PowerTeacher IEP Anywhere Claim Status Form Question 2 23.79g of solid sodium hydroxide, NaOH is added to 87.5 ml of a 1.97M solution of iron(Il) chloride, FeC13. This causes iron(III) hydroxide to precipitate out of solution. The reaction is shown below. Determine the limiting reagent then find the mass of the iron(III) hydroxide precipitate. 3NAOH(s) + FeCl3 (aq) - Fe(OH);(s) + 3NaCl(aq) Question 3 The mixture of which two solutions will result in a precipitate being formed? O LIOH(aq) + Na2SO4(aq) O BaCl2(aq) + NAOH(aq) O Pb(NO3)2(aq) + NaC2H3O2(aq) O Al(NO3)2(aq) + BaCl,(aq) O Al(NO3)2(aq) + LIOH(aq) Question 4 Solid H,S is added to 280 ml of a 0.450M CaCl2 solution until no more Cas is formed (see reaction below). At the end of the experiment 5.50 g of CaS is formed. What is the percent yield for the reaction? Molar Masses: Ca (40.08), S (32.07), CI (35.45) CaCl2 (aq) + H,S(s) 2HC(aq)…
- ENB Assume the densities of all solutions are 1.0 g/ml and their specific heat capacities 4.184 J/g. Experime The enthalpy change of neutralization Part I 3 NH4OH(aq) + HCl(aq)- NH4CI(aq) + H2O(E) 2.1 Equation of reaction: 2.0 M HCI 2.0 M NH.OH Volume Number of moles 0.05 25 ml 25 ml 0.05 Temperature 15 °C 15 °C eaction Initial Temperature,T Final Temperature, T Change in temperature, AT 15 °C 16.5 °C 1.5 °C Calculation of q- in J (q- = - qsa) 2.2 What is the enthalpy change (AH) in kJ.mol, when 1 mol of acid is 2.3 neutralized?What volume of 0.50 M KOH would be required to neutralize completely 500mL of 0.25 M H 3 PO 4 solution?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 atm
- Let's assume that there is 400 μatm of pCO2 in our atmosphere. Assumingthere is nothing else in the water coming from the atmosphere, what is the pH of rainwater in equilibrium with this atmospheric CO2?Assume KH = 5.4x10-2 mol kg-1 atm-1. KC1 = 3.47×10-7 mol2 kg-2 for freshwater rain.Hint: Because rainwater is acidic, it has little/no alkalinity, thus the (H+] = Alk = [HCO3-]Why is rainwater naturally acidic, even in the absence ofpolluting gases such as SO2?Calculate the pH of a 0.10 M solution of sodium hypochlorite (NaClO; Ka 2.90 x 10$). Also, calculate the pH after diluting the solution by 10 times.