Standardization of a sodium hydroxide solution against potassium hydrogen phthalate (KHP) yielded the accompanying results Mass of KHP, g 0.7987 0.8365 0.8104 Volume of NaOH, mL 38.29 39.96 38.51 0.8039 38.29 Calculate the average molarity of the base
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- Question. Determination of percent water (%H₂O) in hydrated FeSO4nH₂O is demonstrated in General Chemistry Laboratory (I), Chem. 105. The following table contains the results collected from the students groups. 1 2 3 4 5 6 (a) Calculate the average number of water molecules (b) %H₂O in each sample. 3.38 3.47 3.35 3.40 3.44 3.41 1.4 1.35 1.35 1.44 1.49 1.39 Mass of water (g) Moles of water Moles FeSO4 11= Moles H₂O Mole FeSO Average n % water in hydrated salt (wt/wt) Hint: Atomic mass: Fe = 56 g/mol; O = 16 g/mol; H = 1.0 g/mol; S = 32 g/mol.What is the percent magnesium hydroxide, if a sample of magnesia magma weighing 5.2430g when dissolved in 25 mL of 0.9915 N H2SO4 required 9.85 mL of 1.4102 N NaOH to titrate the excess acid? Round to 2 decimal point; Answer should be with the correct unit.9:24 PM Mon Feb 21 * 65% A openstax.org Solute concentrations are often described with qualitative terms such as dilute (of relatively low concentration) and concentrated (of relatively high concentration). Concentrations may be quantitatively assessed using a wide variety of measurement units, each convenient for particular applications. Molarity (M) is a useful concentration unit for many applications in chemistry. Molarity is defined as the number of moles of solute in exactly 1 liter (1 L) of the solution: mol solute M = L solution EXAMPLE 3.14 Calculating Molar Concentrations A 355-mL soft drink sample contains 0.133 mol of sucrose (table sugar). What is the molar concentration of sucrose in the beverage? Solution Since the molar amount of solute and the volume of solution are both given, the molarity can be calculated using the definition of molarity. Per this definition, the solution volume must be converted from mL to L: mol solute 0.133 mol M = = 0.375 M L solution 355 mL × 1L…
- To prepare 50 mL solutions of 0.1 M CuSO4 in water (calculation to prepare chemicals in spectrophotometer)You are asked to weigh 2 g of lithium and add it to 1500 ml of distilled water +2drops of indicator, knowing that the density of water is 1 at room temperaturewhile conducting this experiment. After calculating the amount of LiOH, you need to dilute to prepare 0.25 M of LiOH in a 3000 ml solution. Show your calculation and units.Knowing that the initial volume that you used was 1500 ml. Use this equation to calculate ( CLiOH x VLiOH) before dilution = (CLiOH x VLiOH) after dilutionKk.222. I need both parts solution....
- 3. A student neutralized 25.0 cm³ of sodium hydroxide solution with 0,6 student carried out the experiment three times and obtained the following results. Experiment 3 Experiment 1 Experiment 2 Volume of Acid 19.90 17.30 17.40 Used/ cm3 (a) The student calculated the volume of acid used by calculating the average of the volume of acid used in Experiment 2 and Experiment 3. Explain why the first reading was not considered. (b) Calculate the amount (moles) of 0.6 moldm³ sulfuric acid in the average titre value used to neturalise the sodium hydroxide. (c) How many moles of sulfuric acid react with 1 mole of sodium hydroxide? (d) What amount (moles) of sodium hydroxide were there in the 25 cm³ sample?Experiment-A8: Spectrophotometry of Cobalt( Pre-laboratory Exercises 1. (a) Define Beer's law and give the mathematical equation (specify each symbol in the equation). concentration of achemical Solution Beer's Law states that the in the following A = Ebc is directly proportional to its absorption of light & can be calculated formula (b) Briefly explain what Beer's plot is and how do you obtain the Beer's constant (k) from the plot. is a straight line with _ay-intercept Beer's plot of zero & a slope of ab oreb. It represents the absorptunity the length Absorbance 8 can be calculate by multiplying Constant by the path length then dinding that value by the 2. The following solutions are prepared from 0.200 MNICI, and their absorbance measured at 725 nm. Solution # 1 2 3 4 5 Volume (mL) of 0.200 M NiCh 1.00 2.00 3.00 4.00 pride 5.00 Volume (mL) of H₂O 4.00 3.00 2.00 1.00 0.00 INICI] (a) Calculate the molar concentration of NiCl₂ in each solution 1-5. Absorbance at 725 nm 0.105 0.210 0.315…A solution of HCl was titrated against sodium carbonate. What is the normality of acid for Trial 3 in the given data? T1 T2 0.3562 0.3479 0.3042 Weight (g) Initial V (mL) 0.80 1.60 0.40 Final V (mL) 35.20 36.70 39.80 Vol HCI used (ml) 35.10 39.40 N of HC (eq/L) 0.1954 0.1870 Average N of HCl (eq/L)
- A 1.787 g sample containing some Fe2+ ion requires 31.50 ml of a 0.02188 M KMnO4solution to reach a pink endpoint. What is the percent by mass of Fe2+ in the sample?Give handwritten answer PPm=? PPb=?Question . Determination of percent water (%H₂O) in hydrated FeSO4nH₂O is demonstrated in General Chemistry Laboratory (I), Chem. 105. The following table contains the results collected from the students groups. 1 23 2 4 5 6 3.38 3.47 3.35 3.40 3.44 3.41 1.4 1.35 1.35 1.44 1.49 1.39 Q1) Assume MM of FeSO4 is 152 g/mol. What is the average number of water molecules in the samples? Q2) What is the average % water (wt/wt) for all samples? n= Moles H₂O Mole FeSO, Average n Q3) What is the average number of moles of water for all samples? Q4) What is the correct formula of the salt? % water in hydrated salt (ww/wt)