Some projection models put the carbon dioxide concentration at 1255 ppm by the year 2100. Calculate [CO2] in rainwater at this concentration. KH=.034 mol/(L * Atm). Calculate the pH of the rainwater if all the CO2 reacts with water to produce carbonic acid (H2CO3, pKa 3.6) (ignore the partial pressure of water). i need help for this

If a sample of a certain solution is determined to have a pH of 8.9, what is the concentration of [H3O+] in the solution? Write your answer in scientific notation and round the significand to two decimal places. Answer moles/liter Keypad Keyboard Shortcuts

At 25°C the value of Kw is 1.0 x 1014. At 60°C the value of Kw is 1.0 x 1013. Is the reaction exothermic or endothermic? Explain briefly. Calculate [H3O] and pH in a neutral solution at 60°C. 2H,0 0 H,O* (12)+OH (2)

Express the answer to two decimal places. What is the pH of a solution that results from mixing together equal volumes of a 0.130 M solution of acetic acid and a 0.065 M solution of sodium hydroxide? (pKa of acetic acid = 4.75)

1.Carbon occurs in water in 3 different photons, CO2, HCO3', and CO3 2. a- Is there a certain pH value at which carbon occurs in all 3 forms? Yes/NO b- In seawater (pH =8.2) the greatest percentage of carbon occurs in the form HCO3? Yes/NO 2.Carbon can occur in Water in three different fotons (substance) as Carbon dioxide (CO2), hydrogen carbonate (HCO3), or Carbonate ( The pH value of (water indicates how high the percentage of three forms is (substance amount). The diagram shows these substances amount depending on the pH value. 100 80 Hideogen Carbonate 60 Carbon dioxide Carbonate (Co) 20 PH value 10 11 12 13 Which of the following is correct A)ln Seawater (pH value of 8.2) The greatest percentage of carbon occurs in the form of HCO3 B) There is a pH value at which carbon occurs in water in the form of CO, as in the form of HCO3 and CO3 2 a. Only A is correct b. Only B is correct c. Both are correct d. None is correctn dl

The calcium concentration of Lake Mary (a lake in New Hampshire) is 4 x 10-4M. Estimate the pH of this lake? Assume that calcium inputs to this lake are exclusively from calcium carbonate weathering

Determine the pH of the following solutions: 1.    [H+1] = 2.3 X 10-13 M   2.    [H+1] = 7.3 X 10-3  M From the answers you obtain, answer the following questions about each solution: 1.  Determine whether each solution is an acid or base.  Explain your answer. 2.  Determine the potential products of the reaction of the solution identified as acid from above and metallic zinc. 3.  Determine what color litmus paper will turn for each solution. 4.  Determine whether each solution is a (strong acid or base) or a (weak acid or base).

Question: 1 .HA is a weak acid. Its ionization constant, Ka, is 1.3 x 10-13. Calculate the pH of an aqueous solution where the initial concentration of NaA is 0.050 M. 2 . Place 0.112 mol of a weak acid, HA, in enough water to make 1.00 L of solution. The final pH of this solution is 1.29. Calculate the ionization constant, Ka, of HA. 3 . Place 0.648 mol of a weak acid, HA, and 13.1 g of NaOH in enough water to produce 1.00 L of solution. The final pH of this solution is 4.76. Calculate the ionization constant, Ka, of HA. Please complete answers than rating helpful other wise un helpful

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?

The equilibrium constant for an acid is called the acid ionization constant (Ka). If acetic acid (weak acid, HC2H3O2) is placed into water, it ionizes to H+ and C2H3O2- with a Ka of 1.82 x 10-5. Determine the pH of the solution when 20.0 g HC2H3O2 (s) is added to water, with a final volume of 1000. mL?