100 μL of 0.01 mol dm 3 sodium fluoride and 10 mL of pH buffer were added to a 100 mL volumetric flask and made to volume with distilled water. Calculate the concentration of sodium flluoride in the new solution.
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- Potassium acid phthalate, KHC8H4O4 ( MM=204.2 ), reacts with sodium hydroxide on a 1:1 molar basis. A sample of the acid weighing 0.4823 g was titrated with NaOH, requiring 24.35 mL to reach the endpoint. Calculate the molar concentration of the sodium hydroxide solution.If 25,0 cm3 of the NH3 (concentration 0,10 mol∙dm–3) is titrated with the HCl (concentration 0,050 mol∙dm–3), calculate the pH at the equivalence point of the titrationConsider the titration illustrated in Figure 8.] Anhydrous sodium carbonate (Na₂CO₃) is a primary standard. When 0.364 grams of the substance is placed in a conical flask, then 20.00 cm³ of sulphuric acid (H₂SO₄) solution is required to reach the end point of the titration. What is the concentration in mol·dm⁻³ of the sulphuric acid solution? [Give the answer to 3 decimal places. Do not type in the unit. Use a decimal point.] *
- Show how the composition of an aqueous solution that contains 30 mmol dm-3 tyrosine varies with pH.The solubility of borax, which is made up of sodium tetraborate (Na2B4O5(OH)4 8H2O), was analyzed. The dissolution of borax is: Na2B4O5(OH)4 • 8H2O(s) ⇌ 2 Na+(aq) + B4O5(OH)42–(aq) + 8 H2O(l) A 50 mL saturated solution was prepared. After filtration of solution, 5 mL aliquot was transferred to a flask and titrated using 0.432 M HCl. The endpoint was found to be 4.73 mL of the titrant. Tetraborate anion (B4O5(OH)42-) is a weak base which reacts with HCl like the following reaction: B4O5(OH)42–(aq) + 2 H+(aq) + 3 H2O(l) ⇌ 4 H3BO3(aq) What is Ksp expression for the dissolution? What is the tetraborate ions concentration in the filtrate? What is the molar solubility and Ksp of borax if the titration was done at room temperature (298 K)?The researcher extracts a sample of well water and prepares it for TXRF analysis with a 10.00 mg/L V internal standard, like the calibration standards. The result produces SCa = 69297.81 and SV = 13481.2.Determine the concentration of Ca.
- Derive a general expression that shows pH dependence of the distributioncoefficient defined in (2-20) for a weak acid between a fermentation broth and an organic solvent.Calculate the ionic strength of a solution that is 0.040 mol kg−1 in K3[Fe(CN)6](aq), 0.030 mol kg−1 in KCl(aq), and 0.050 mol kg−1 in NaBr(aq).A pharmacist mixes 100 mL of 38% w/w hydrochloric acid with enough purified water to make 360 mL. If the specific gravity of hydrochloric acid is 1.20, calculate the percentage strength (w/v) of the
- Ferric oxide (Fe2O3, density 5 5.24 g/mL) obtained from ignition of a gravimetric precipitate weighed 0.296 1 g in the atmosphere. What is the true mass in vacuum?The mobility of a chloride ion in aqueous solution at 25 °C is 7.91 x 10-8 m2 s-1 V-1. Calculate its molar ionic conductivity.An impure sample of calcium carbonate with a mass of 7.95 g was reacted with 50.00 cm3 of 1.00 mol dm hydrochloric acid (an excess). The resulling solution was transferred to a volumetric flask and titrated with 11.10cm3 of 0.300 mol dm-3 sodium hydroxide solution. Determine the percentage purity by mass of the calcium carbonate sample.CaCO3 + HCl -> CaCl2 + H2O + CO2 HCl + NaOH -> NaCl +H2O a. Determine how many moles of hydrochloric acid were used.b. Determine how many moles of excess HCI was titratedc. Determine how much in moles calcium carbonate present in the sample.d. Calculate the mass of calcium carbonate presente. Determine the percentwge calcium carbonate is in the sample.