An indicator was not used during potentiometric titration of a weak acid Is there a positive error, negative error, no effect, or error could not be determined In terms of the Computed pKa of the unknown weak acid?
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An indicator was not used during potentiometric titration of a weak acid
Is there a positive error, negative error, no effect, or error could not be determined
In terms of the Computed pKa of the unknown weak acid?
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- Blank correction is not done in a Mohr titration of NaCl. Is there a positive error, negative error, no effect, or error could not be determined In terms of the unknown Cl concentration?Three-point calibration was not performed on the pH meter prior to titration. Is there a positive error, negative error, no effect, or error could not be determined In terms of the Computed pKa of the unknown weak acid?How the pH at the equivalence point is determined by the species present; why the pH at the midpoint of the buffer region equals the pKa of the acid
- Direct titration: 10.90 ± 0.02 mL of an unknown KHP solution required 11.72 ± 0.02 mL of 0.1090 ± 0.0006 M NaOH to reach the end point. What is the concentration of KHP in the unknown solution reported with absolute uncertainty? If the unknown solution was prepared by dissolving 5.128 g of the unknown KHP (204.22 g/mol) in 100.00 mL of water, what is the weight percent of KHP in the sample?At the half-way point in the titration of a weak acid with a strong base the pH was measured as 5.16. What is the acidity constant and the pKa of the acid? What is the pH of the solution that is 0.025 M in the acid?a) In the titration of a weak acid with a strong base what is the pH at the 50% equivalence point? The pKa of the weak acid is 4.04. The correct answer should be reported to two places past the decimal. b) What will be the pH at the 62 % equivalence point in the titration of a weak acid with a strong base. The pKa of the weak acid is 4.2. Your answer should be to two places past the decimal (i.e. 0.00)
- Part A: Standardization of a Sodium Hydroxide Solution Titration 1 Titration 2 Titration 3 Mass of 125 mL flask 45.849g 46.715g 44.953g Mass of flask and KHP 46.849g 47.745g 46.003g Initial buret reading (mL) 0.5 ml 0.5 ml 0.5 ml Final buret reading (mL) 27.8 ml 26.5 ml 26.7 ml Volume of NaOH used (mL) 45.11 ml 45.06 ml 45.14 ml Calculations Titration 1 Titration 2 Titration 3 Moles of KHP Moles of NaOH Molarity of NaOH Average Molarity of NaOH: _______________It is a solution of unknown concentration in which a solution of accurately known concentration is gradually added until the reaction is complete. Analyte Endpoint Indicator TitrantDo you always have to use a primary standard in the standardization of titrant? Why or why not?
- What is a primary reason for needing to standardize strong base titrants like KOH? Select the single best answer. OKOH is not very soluble in aqueous solutions, thus making the concentrations difficult to determine. KOH reacts with moisture in the air, thereby making accurately-determined concentrations of their solutions difficult. O Standardization is the process of reacting a strong base, like KOH, with an acid. O Standardization is the process of dissolving KOH in aqueous solution. OKOH is a very inexpensive, highly soluble, and easy-to-use base.Identify the definition of a primary standard in titration? Identify the characteristics of a substance to be considered as a primary standardA standard serum sample containing 102 meq/L chloride was analyzed by coulometric titration with silver ion. Duplicate results of 101 and 98 meq/L were obtained. (a) Calculate the mean error (b) Calculate the relative error (c) Calculate the relative accuracy