A sodium hydroxide solution is to be standardized using KHP (99.5% purity, MW = 204.22). A 1.500-g KHP dissolved in water required 14.84 ml of NaOH solution for the phenolphthalein endpoint. Calculate the molarity of the NaOH solution.
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- Transfer 0.5 mL phenolphthalein to a flask 25 mL KHP. Then transfer 13.2mL NaOH in the KHP that make it be pink. As the picture shows. Now, show a complete calculation for the concentration of the sodium hydroxide solution.A 2.190 g sample of a solid mixture containing only potassium carbonate (MM=138.2058 g/mol) and potassium bicarbonate (MM=100.1154 g/mol) is dissolved in distilled water. A volume of 30.74 mL of a 0.778 M HCl standard solution is required to titrate the mixture to a bromocresol green end point. Calculate the weight percent of potassium carbonate and potassium bicarbonate in the mixture. K2CO3: ? wt% KHCO3: ? wt%-3 . The densities of pure water and ethanol are 997 and 789 kg · m respectively. The partial molar volumes of water and ethanol are 17.8 × 10-³ and 55.2 × 10-³ L.mol-¹, respectively. Part A Calculate the change in volume relative to the pure components when 3.25 L of a solution with Tethanol = 0.524 is prepared. Express your answer to two significant figures and include the appropriate units. AV = 3.24 μà L ?
- (A) if both sentences are true,(B) if both sentences are false,(C) if the first sentence is true but the second is false, and(D) if the first sentence is false but the second is true. 1. In the Winkler Titration Method, sodium thiosulfate is standardized against a known concentration of magnesium iodate. The normality (N) of a solution is always equal to its molarity (M). 2. In the experiment on determining the dissolved oxygen concentration of a water sample, the compound used to acidify the sample was hydrochloric acid. An acidic solution will have a pH greater than 7. 3. Radioactive wastes, like uranium, must be handled and disposed of according to special regulations designed to protect people and the environment. Nuclear power plants produce too much greenhouse gases due to the burning of uranium.A chemist receive different mixtures for analysis with the statement that it contain NaOH, NaHCO3 , Na2CO3 or compatible mixtures of these substances together with the inert material. From the data given, identify the respective materials and calculate the percentage of each component. 1.000g samples and 0.2500 N HCl were used in all cases. Sample 1 With phenolphthalein as the indicator, 24.32 ml of HCl was used. A duplicate sample required 48.64 ml HCl using methyl orange as the indicator. Sample 2. With phenolphthalein as the indicator it uses 28.2 ml of HCl to make it colorless and added with methyl orange indicator and uses 11.3 ml of HCl to reach the end point.2. A sodium hydroxide solution is to be standardized using KHP (99.5% purity, MW = 204.22). A 1.500-g KHP dissolved in water required 14.84 ml of NaOH solution for the phenolphthalein endpoint. Calculate the molarity of the NaOH solution.
- A 25.190 g sample of aqueous waste leaving a fertilizer manufacturer contains ammonia. The sample is diluted with 74.348 g of water. A 10.405 g aliquot of this solution is then titrated with 0.1058 M HCI. It required 28.58 ml. of the HCI solution to reach the methyl red endpoint. Calculate the weight percent NH, in the aqueous waste. wt% NH, %3D Potassium hydrogen phthalate (KHP) is often used as a primary standard in acid-base titrations. If 19.15 ml.L NAOH is required to neutralize 0.427 g KHP, what is the concentration of the NaOH? M concentration:To determine the Kgp of barium oxalate at 12°C, a 100.0 mL saturated solution was prepared by adding the solid in distilled water maintained at 12°C until it no longer dissolves. The solution was filtered and from this, a 10.0 mL aliquot of the filtrate was drawn. It was found out that 10.70 mL of 5.60 x 104 M HCI was used to reach the endpoint. Given that two moles of HCl react for every mole of dissolved oxalate during the titration, determine the amount of dissolved oxalate in the titration flask (in mol/L). Do not include the unit in your answer below. For those who will be using scientific notation, please follow the format below: Example: 0.00487 -> 4.87E-3 58000 -> 5.8E+4A solution is saturated with magnesium palmitate [Mg(C16H31O2)2, a component of bathtub ring] at 50°C. How many milligrams of magnesium palmitate will precipitate from 956 mL of this solution when it is cooled to 25°C? For Mg(C16H31O2)2, Ksp = 4.8 x 10–12 at 50°C and 3.3 x 10–12 at 25°C.
- A 0.1530 g of pure KIO3 was dissolved in 50 mL distilled water. This was then added with KI and 6N H₂SO4. After allowing the said solution to stand in the dark for 3 minutes, this was then titrated to end point with 31.35 mL sodium thiosulfate solution, with starch as the indicator. What is the normality of the sodium thiosulfate solution? Atomic weights: K = 39.1 1= 126.9 O= 16.0ST5G.1- What is the approximate solubility [in units of MILLImolar] of an ionic compound M2X3 with ions M3+ and X2- if Kg = 5.6*10-7? The values for Kg and ion charges may be %3D unrealistic for the sake of problem-solving variety and ease-of-use in Canvas. Type your answer..Suka-tuba is a vinegar variety derived by fermenting the sap of a coconut tree. You are tasked to analyze its acetic acid Describe the preparation of 5.0 M NaOH stock solution from analytical grade NaOH pellets. Describe the preparation of 0.10 M NaOH solution from the stock solution. How much KHP was used per trial. (purity KHP: 99.0%).