Buffer Calculations
Buffer calculations play a pivotal role in various fields, from chemistry to computer science, offering a systematic approach to maintain stability and optimize performance. In chemistry, buffers ensure pH stability, crucial for enzymatic reactions and biological processes. Similarly, in computing, buffer calculations optimize memory allocation, enhancing system efficiency and preventing data overflow. Understanding buffer calculations involves grasping fundamental principles of equilibrium and resource management, making it indispensable in both scientific and technological domains. This introductory exploration sets the stage for delving deeper into the intricacies of buffer systems and their applications across diverse disciplines.
Questions
- How do you calculate the pH of a buffer?
- How to calculate the ratio of sodium carbonate and sodium bicarbonate in 'x' Molar sodium carbonate-sodium biocarbonate buffer?
- A buffer solution was prepared from #0.615*L# of weak acid #HA# at #0.250*mol*L^-1# concentration, and a #0.500*L# volume of #NaOH# at #0.130*mol*L^-1# concentration. What is the resultant #pH# of this buffer?
- What is an example of a pH buffer calculation problem?
- A 1.00 L buffer solution is 0.150 M in #HC_7H_5O_2# and 0.250 M in #LiC_7H_5O_2#. How do you calculate the pH of the solution after the addition of 100.0 mL of 1.00 M #HCl#? The Ka for #HC_7H_5O_2# is #6.5 × 10^–5#.
- What is the pH of a solution made of 0.1 M acetic acid and 0.1 M potassium acetate to which 0.001 mol of KOH has been added?
- You are asked to make a buffer solution with a pH of 2.0. Use the information below to identify an appropriate choice of an acid and a conjugate base to make the buffer?
- What is the set of chemical equations that describe the buffering action of phosphate buffered saline (PBS)? Calculate theoretically the pH of phosphate buffered saline.
- A buffer was prepared by adding 20g of acetic acid #CH_3COOH# and 20g sodium acetate to enough water to make a 2.0L solution.Determine the pH and write an equation for reaction when a few drops of #HCl# are added to the buffer?
- What are the different types of buffering system in the body?
- Calculate the #"pH"# change in a buffer solution upon the addition of strong acids / base of known concentration?
- How would you use the Henderson-Hasselbalch equation to calculate the pH of a buffer solution that is 0.27 M in formic acid (#HCO_2H#) and 0.50 M in sodium formate (HCO_2Na)?
- Why are buffer solutions used to calibrate pH?
- How does the dilution factor affect a buffer solution?
- A #"25.0-mL"# sample of #"0.150-mol L"^(-1)# hydrofluoric acid is titrated with a #"0.150-mol L"^(-1)# #"NaOH"# solution. What is the #"pH"# after #"26.0 mL"# of base is added?
- The concentration of carbonic acid in normal blood is 0.029 mol/L and the pKa for carbonic acid is 6.1. Using the Henderson-Hasselbach equation, how do you determine the concentration of bicarbonate ion in normal blood sample which is pH 7.40?
- A beaker with 120mL of an acetic acid buffer with a pH of 5.00 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.1M. A student adds 6.60mL of a 0.300M HCl solution to the beaker. How much will the pH change?
- What are the "Universal" buffer mixtures?
- A buffer is made by dissolving #"NaClO"# and #"HClO"# in water. How do you write equations to show how this buffer neutralizes added H+ and OH-?
- If a buffer solution is 0.290 M in a weak base (#K_b = 6.4 xx 10^(-5)#) and 0.520 M in its conjugate acid, what is the pH?