estimate the pH of water that contains .62 mg/L of carbonic acid. assume that [H+]=[HCO3-] at equilibrium and that the dissociation of water may be neglected. the water temperature is 25C. molecular weight of H2CO3=62g/mol.
estimate the pH of water that contains .62 mg/L of carbonic acid. assume that [H+]=[HCO3-] at...
What is the pH of rainwater in pristine environments? Assume the temperature is 25°C, the total pressure is 1 atm and the rainwater is in equilibrium with the atmosphere. Solution: 5 species are present in the aqueous phase H2CO3(aq), HCO3-(aq), CO3-2(aq), H+ and OH- Equations: 1H2CO3 → H+ + HCO3- (carbonic acid dissociation) K1 = [H+][HCO3-]/[H2CO3] = 4.47 x 10-7M
a) Find the concentration of H+, HCO3- and CO32-, in a 0.01M solution of carbonic acid if the pH of this is 4.18. Ka1 (H2CO3) =4.45 x 10–7 and Ka2 =4.69 x 10–11 (b) Calculate the pH at the equivalence point of the titration between 0.1M CH3COOH (25 ml) with 0.05 M NaOH. Ka (CH3COOH) = 1.8 x 10–5.
The following questions is based on ionization of carbonic acid. [H2CO3 = H+ + HCO3- K1 = 4.7 X 10-7, pK1 = 6.34 ] [HCO3- = H+ CO3-2 K2 = 4.4 X 10-11, pK2 = 10.36] Calculate the pH ofthe solution form by mixing the following: a)50.0ml of 0.100 M H2CO3 with 50.0ml of 0.050 M NaOH . b)50.0ml of 0.100 M H2CO3 with 50.0ml of 0.150 M NaOH . c)50.0ml of 0.100 M H2CO3 with 50.0ml of 0.100 M...
Carbonic acid (H2CO3) is unstable in water and rapidly decomposes i to CO2(g) and H2O(l). Consequently, the reaction between Coc-H+(aq) and HCO3-(aq) is better represented as
A water with a pH of 9.0 contains 20 mg/L CO3-2 and 55 mg/L HCO3-. Calculate the alkalinity of the water expressed as meq/L (milli equivalents per liter) and as mg/L as CaCO3.
8. (4 pts) The biological catalyst carbonic anhydrase converts carbon dioxide to carbonic acid, an essential component of the bicarbonate buffer system regulating our blood pH. What mass (in me) of sodium carbonate (NaHCO, MM: 84.006 g/mol) must be added to 500.0 ml of 0.029 M carbonic acid (K. 1 4.3 x 10-7, K., 4.8 x 10-11) to produce a solution with pH = 7.40? Assume no volume change after the addition of sodium carbonate. H2CO3 + H2O=HCO3 + H20...
1a.) From water sample, 10 mg/L HCO3- as CaCO3, 10 mg/L CO3- as CaCO3 and 50 mg/L Ca+ as CaCO3 were measured. pH was near neutral. What is alkalinity? _____ mg/L as CaCO3 1b.) From water sample, 10 mg/L HCO3- as CaCO3, 10 mg/L CO3- as CaCO3 and 50 mg/L Ca+ as CaCO3 were measured. pH was near neutral. What is alkalinity? _____ mg/L as CaCO3 1c.) Calculate Ksp = _____ A2BO3 ->2A++ BO32- Molar concentration of A+ = Molar...
If the concentration of carbonic acid (H2CO3) in sea water is equal to 5.5 x 10^-4 mol L, is this concentration in equilibrium with P(co2) in the atmosphere?
Consider the acid dissociation behavior of carbonic acid, H, COZ. pKa1 = 6.351 PK22 = 10.329 HO - ¢=o C=0 HO 0 pH . What is the predominant species present at pH 6.82? OH,CO2 O coz- OHCOZ [CO3-) Calculate the ratio - at pH 9.85. [HCO3]"} [CO2-). [HCO3]
helpp!! The pH of a 0.57 M solution of carbonic acid (H,CO2) is measured to be 3.30. Calculate the acid dissociation constant K of carbonic acid. your answer to 2 significant digits. ş Complete the table below. Round each of your entries to 2 significant digits. You may assume the temperature is 25 °C. conjugate base conjugate acid formula K formula X 5 ? нсо, 2.2 x 10 NH 3.6 × 10 -10 HONH LIX 10 Order these chemical species...