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![The pH of blood is given = 7.40 Carbonic acid concentration [HA] -0.0010M ka of carbonic aud= 4.38107 As we know pka = log (k](http://img.homeworklib.com/questions/3d0e89a0-cfd0-11eb-8e19-51c6776eec4d.png?x-oss-process=image/resize,w_560)
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Carbonate buffers are important in regulating the pH of blood at 7.40. If the carbonic acid...
(a) Carbonate buffers are important in regulating the pH of blood at 7.40. what is the...
(a) Carbonate buffers are important in regulating the pH of blood at 7.40. what is the concentration ratio of CO2 (usually written H2CO3) to HCO3-in blood at pH = 7.40? H2CO3(aq)-HCO3-(aq) + H+(aq) Ka = 4.3 × 10-7 [H2CO3] / [HCO3-]- (b) Phosphate buffers are important in regulating the pH of intracellular fluids at pH values generally between 7.1 and 7.2. What is the concentration ratio of H2Po4 to HPO2 in intracellular fluid at pH = 7.15? H2PO4(aq)HPO42(aq)H(aq) Ka =...
please answer as soon as possible Student Name section # Student ID# Date 1. A student...
please answer as soon as possible
Student Name section # Student ID# Date 1. A student was asked to prepare three solutions and to calculate their pH: Solution A: 0.24 M of NH3 and 0.20 M of NHACI Solution B: adding 0.005 mol of NaOH to 0.50 L of solution A Solution C: adding 0.030 mol of HCl to 0.50 L of solution A a. Calculate the pH of these solutions. (NHA"; K, -5.6x101) b. What property for buffered solutions...
One of the most important buffering systems in the biological realm is the carbonic acid (H2CO3)/carbonate...
One of the most important buffering systems in the biological realm is the carbonic acid (H2CO3)/carbonate ion (HCO3- ) system that maintains the pH of blood plasma to a relatively constant value. In blood at 37°C, the Ka of carbonic acid is 8x10-8. Suppose that the concentrations of the buffer components in the blood plasma are: [HCO3-] = 0.24 M and [H2CO3] = .12 M. Calculate the pH of blood.
8. The normal pH of human blood is about 7.4. The carbonate buffer system in the blood uses the following reaction:...
8. The normal pH of human blood is about 7.4. The carbonate buffer system in the blood uses the following reaction: CO2(+ 2H2O() H2CO3(aq) HCO3(aq) + H:04) The concentration of carbonic acid, H2CO3, is approximately 0.0012M and the concentration of the hydrogen carbonate ion, HCO3 is around 0.024M. Calculate the pH of blood
8. (4 pts) The biological catalyst carbonic anhydrase converts carbon dioxide to carbonic acid, an essential...
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...
The pH of a bicarbonate-carbonic acid buffer is 6.62. Calculate the ratio of the concentration of...
The pH of a bicarbonate-carbonic acid buffer is 6.62. Calculate the ratio of the concentration of carbonic acid ( H2CO3 ) to that of the bicarbonate ion ( HCO3− ). ( Ka1 of carbonic acid is 4.2 × 10−7. ) [ H2CO3 ]/ [ HCO3− ] =
The pH of a bicarbonate-carbonic acid buffer is 5.96. Calculate the ratio of the concentration of...
The pH of a bicarbonate-carbonic acid buffer is 5.96. Calculate the ratio of the concentration of carbonic acid (H2CO3) to that of the bicarbonate ion (HCO3−).(Ka1 of carbonic acid is 4.2 × 10−7.) [ H2CO3 ] [ HCO3− ] =
The pH of blood plasma is 7.40. The principal buffer system is HCO3?/H2CO3. Calculate the ratio...
The pH of blood plasma is 7.40. The principal buffer system is HCO3?/H2CO3. Calculate the ratio [HCO3?]/[H2CO3] in blood plasma. (Ka of H2CO3, carbonic acid, is 4.5 × 10?7) Enter your answer in the provided box.
Buffers are common (and extremely important) in biological systems, including in human body. One of the...
Buffers are common (and extremely important) in biological systems, including in human body. One of the most important biological buffers in human blood is the buffer established between carbonic acid and bicarbonate ion (H2CO3/HCO3–). At 25 oC, H2CO3 has a Ka1 of 4.45x10–7 and a Ka2 of 4.69x10–11. a. Will Ka1 or Ka2 of H2CO3 be instrumental in determining blood pH? Briefly explain your reasoning. b. Let’s pretend that there was an equal ratio of carbonic acid to bicarbonate (note...
One of the buffers to maintain the pH of blood is the carbonic acid, H_2CO_3, buffer....
One of the buffers to maintain the pH of blood is the carbonic acid, H_2CO_3, buffer. Carbonic acid is diprotic and it's equilibrium constants are K_a1 = 4.2 times 10^-7 and K_a2= 4.8 times 10^-11. How would you prepare 5.0 L a carbonic acid buffer of a pH of 7.2 from 0.250 M H_2CO_3? You have available NaHCO_3 (MW = 84.0) and Na_2CO_3 (MW = 106).
(a) Carbonate buffers are important in regulating the pH of blood at 7.40. what is the concentration ratio of CO2 (usually written H2CO3) to HCO3-in blood at pH = 7.40? H2CO3(aq)-HCO3-(aq) + H+(aq) Ka = 4.3 × 10-7 [H2CO3] / [HCO3-]- (b) Phosphate buffers are important in regulating the pH of intracellular fluids at pH values generally between 7.1 and 7.2. What is the concentration ratio of H2Po4 to HPO2 in intracellular fluid at pH = 7.15? H2PO4(aq)HPO42(aq)H(aq) Ka =...
please answer as soon as possible
Student Name section # Student ID# Date 1. A student was asked to prepare three solutions and to calculate their pH: Solution A: 0.24 M of NH3 and 0.20 M of NHACI Solution B: adding 0.005 mol of NaOH to 0.50 L of solution A Solution C: adding 0.030 mol of HCl to 0.50 L of solution A a. Calculate the pH of these solutions. (NHA"; K, -5.6x101) b. What property for buffered solutions...
8. The normal pH of human blood is about 7.4. The carbonate buffer system in the blood uses the following reaction: CO2(+ 2H2O() H2CO3(aq) HCO3(aq) + H:04) The concentration of carbonic acid, H2CO3, is approximately 0.0012M and the concentration of the hydrogen carbonate ion, HCO3 is around 0.024M. Calculate the pH of blood
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...
One of the buffers to maintain the pH of blood is the carbonic acid, H_2CO_3, buffer. Carbonic acid is diprotic and it's equilibrium constants are K_a1 = 4.2 times 10^-7 and K_a2= 4.8 times 10^-11. How would you prepare 5.0 L a carbonic acid buffer of a pH of 7.2 from 0.250 M H_2CO_3? You have available NaHCO_3 (MW = 84.0) and Na_2CO_3 (MW = 106).
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