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How do you convert a pH value into a value for [H3O+]? and how you do...
Based on the data on the first page, how do you calculate
H3O+, the concentration of molecular form of acid or base at
equilibrium and the value of Ka or Kb?
Report Data Part I: Determination of Ka or Kb for an UninotiT solution Unknown number: Concentration of unknown: ON (0.100 M, unless you are told otherwise) pH: S.29 Part II: Preparation of a Buffer Solution Target pH for the buffer 568 Perform calculations related to the preparation of the...
How do you calculate the pH of a solution containing a weak acid or a weak base? Please write down the general formula for finding the H3O+ ion concentrations in case of a weak acid Please explain the common-ion effect in terms of Le Châtelier. You might want to use the general chemical equation for an acid ionization HA + H2O ↔ A- + H3O+ to help you explain the phenomenon. How do you calculate the degree of ionization? Please...
You can also do the reverse, calculate the H3O+ molarity from the pH, using the formula, H3O+ molarity = 10^-pH What is the H3O+ molarity of a solution having the pH of 2.37?
The pH value is an expression of the molarity of H3O+ ions in solution. This concentration has strong impact on chemical reactions. The molarity is very small value, and therefore awkward to use. The pH scale simplifies this concentration making communication easier and faster. Demonstrate the relationship between pH and H3O+ molarity, using the formula, pH = -log(H3O+) where () indicates concentration in molarity of a substance. What is the pH of a solution, having the H3O+ concentration of 0.00038...
answer the following in a complete sentence or two (1)how do you know if an acid is strong or weak 2))how do youcalculate pH of a strng acid (3))how do youcalculate the pH of a weak acid solution (4) if you know Ka of an acid how do you determine the kb of its conjugate base 5)if you know[OH-]for solution ,how do you determine [h3o+]. Answer with proper explanation
Base/Acid Ratios in Buffers Just as pH is the negative logarithm of [H3O+], pKa is the negative logarithm of Ka, pKa=?logKa The Henderson-Hasselbalch equation is used to calculate the pH of buffer solutions: pH=pKa+log[base][acid] Notice that the pH of a buffer has a value close to the pKa of the acid, differing only by the logarithm of the concentration ratio [base]/[acid]. Part A Acetic acid has a Ka of 1.8
2. Calculate the pH, pOH, [H3O+], and [OH-] of a 0.30 M solution of the weak acid, hypobromous acid, HOBr. The Ka value for HOBr is 2.8 x 10-9.
Calculate [H3O+] for each solution given its pH: pH = 1.06, pH = 3.98, pH = 8.53, pH = 12.52. Please explain in detail as I'm lost on how to do these. TIA
Determine the PH and [h3o+] in a .265 M HClO solution. The Ka of HClO is 2.9x10^-8
Determine the H3O+ concentration in a solution having a pH value of 7.77.