Show Your Calculations Show at least one example calculation for determining pH for the buffer and one for determining pH of H,O. + log Base PH - Pka acid
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- 2,5 ml volume has taken from an “hypothetic” solution which includes (3+) Sb and (3+) Fe and at the titration with 0.1004 N KMnO4, the wasted amount has found as 16,4 mL. The other 2,5 mL that has taken, has reduced with Zn after that, this 2,5 mL solution has titrates with the same KMnO4 solution solution and the wasted amount is 26,5mL. With these datas find the %concentrations of the ions at the solution.Data Table 1: Complexometric Titration of Hard Water 6ml of water used (5ml of hard water and 1ml of buffer) Hard Water Trial 1 Hard Water Trial 2 Hard Water Trial 3 Initial Syringe Reading (mL) 1ml 1ml 1ml Final Syringe Reading (mL) 0.55ml .50ml .33ml Volume of EDTA Consumed (mL) 0.45ml .50ml .77ml Water Hardness ppm CaCO3 (mg/L) Average ppm CaCO3 (mg/L): photo shows equation that needs to be used to solveData Table 3: Complexometric Titration of Soft Water 6ml of water used (1ml of buffer and 5ml of soft water) Hard Water Trial 1 Hard Water Trial 2 Hard Water Trial 3 Initial Syringe Reading (mL) 1ml 1ml 1ml Final Syringe Reading (mL) 77ml 79ml 75ml Volume of EDTA Consumed (mL) .23ml .21ml .25ml Water Hardness ppm CaCO3 (mg/L) Average ppm CaCO3 (mg/L):
- A buffer was made by mixing 0.1886 moles of CH3CH2CO2H with 0.1517 moles of KCH3CH2CO2 and diluting to exactly 1 liter. What will be the pH after addition of 10.00 mL of 0.2441 M HBr to 50.00 mL of the buffer? Ka(CH3CH2CO2H) = 1.300e-5. Note: only a portion of the original buffer is used in the second part of the problem. Key Concept: Buffers resist pH change and are prepared by mixing the conjugate acid and base together. Addition of either a strong acid or a strong base will cause a small shift in pH to a lower or higher pH, respectively.Strategy: Determine the moles of HA and A− the buffer prior to addition of either a strong acid or base by multiplying by the molarity and volume (50 mL) → determine mole of strong acidadded to the buffer. Adjust the moles to account for loss of conjugate base and formation of conjugate acid with addition of a strong acid or loss of conjugate acid and formation of conjugate base with addition of a strong base → use Henderson-Hasselbach equation to…A RbOH solution is titrated four (4) times against potassium hydrogen phthalate (KHP; FW=204.224) samples to the Phenolphthalein endpoint. Using the data below, determine the concentration of the RbOH solution? g of KHP Volume of Base Required 0.5373 g 42.49 mL 0.5856 g 43.88 mL 0.5790 g 48.56 mL 0.5856 g 44.60 mL (Report your answer as "mean +/- std dev") M What is the percent relative standard deviation? % What is the 99% Confidence Interval for the concentration of the solution (population mean)?The data from my observations is given below: Concentration of Standardized NaOH - 1.00 mol/L Mass concentration of acetic acid - 2.40 g/L Trial 1 Trial 2 Measured pH of the acetic acid solution 3.07 3.05 Mass of acetic acid solution taken for titration 20.0 g 20.0 g Initial buret reading of NaOH titrant 0.00 mL 0.00 mL Final buret reading of NaOH titrant 0.82 mL 0.79 mL Net volume of NaOH 0.82 mL 0.79 mL Millimoles of NaOH to end point of titration 0.82 mmol 0.79 mmol Millimoles of acetic acid in sample 0.82 mmol 0.79 mmol Molar concentration of acetic acid solution 0.043 mol/L 0.041 mol/L Calculated molar mass of acetic acid g/mol g/mol Average molar concentration of acetic acid for the samples titrated: 0.042 mol/L Average pH: 3.06 Question: Calculate the corresponding [H3O+], compute the corresponding concentration of A- and HA, and calculate the dissociation constant Ka Thank you!
- A 250.00 mL solution of 0.00215 M AB4 is added to a 230.00 mL solution of 0.00380 M C3D2. What is pQsp for A3D4? Answer: (18.607)14. A 130.00 mL solution of 0.00335 M A3B4 is added to a 160.00 mL solution of 0.00105 M C3D4. What is pQsp for A3D4?Titration of 50.00 mL of 0.04715 M Na2C2O4 required 39.25 mL of a potassium permanganate solution.MnO4- + 5H2C2O4 + 6H+ → 2Mn2+ + 10CO2(g) + 8H2OCalculate the molar concentration of the KMnO4 solution.
- 4. The molar absorptivities of the indicator weak acid HIn (K_{a} = 1.42 * 10 ^ - 5) and its conjugate base In at 570 were determined as epsilon(HIn) = 7120 and ε(In) = 961. The optical length b = 1.00 cm. (a) What is the absorbance of an unbuffered indicator solution having total indicator concentration 8.0 * 10 ^ - 5 (b) What is the absorbance of a buffered indicator solution having total indicator concentration 8.0 * 10 ^ - 5 and pH = 6.5 .Data Table 2: Complexometric Titration of Tap Water photo shows equation to find water hardness 6 ml of water used (5 ml of tap water 1ml of buffer) Hard Water Trial 1 Hard Water Trial 2 Hard Water Trial 3 Initial Syringe Reading (mL) 2ml 2ml 2ml Final Syringe Reading (mL) .61ml .69ml .58ml Volume of EDTA Consumed (mL) 139ml 131ml 142ml Water Hardness ppm CaCO3 (mg/L) Average ppm CaCO3 (mg/L):A 50.00 (±0.02) mL portion of an HCl solution required 29.71(±0.02) mL of 0.01963(±0.0032) M Ba(OH)2 to reach an end point with bromocresol green indicator. ? of HCL = 29.71?? ? 0.01963 ???? ??(??)2 ?? ? 2 ???? ??? ???? ??(??)2/ 50.00?? = 0.02333 ? Calculate the uncertainty of the result (absolute error).Calculate the coefficient of variation for the result.