Q: Titration of a 20.0 mL sample of acid rain required 1.7 mL of 0.0811 M NaOH to reach the end point.…
A: Molarity is defined as moles of solute present per liter kf a solution. molarity=moles of…
Q: Which among the following is not a base?
A: Arrhenius base is the chemical species that increases the OH- ion concentration in the aqueous…
Q: In one trial of the standardization of a Na2S2O3 solution, a 10.00 mL volume of 5.00×10-3 M KIO3 is…
A: Given data is as follows: The volume of KIO3 = 10.00 mL The concentration of KIO3 = 5.00×10-3 M The…
Q: Standardization of a sodium hydroxide solution against potassium hydrogen phthalate (204.2 g/mol)…
A: First, calculate the moles of KHP: Moles of KHP = mass/molar mass = 0.8365g/(204.2gmol-1) = 0.004096…
Q: In the titration calculation, moles of KOH were calculated from the known molarity and measured…
A: Given : moles of succinic acid has been calculated in the procedure To find : mass of Succinic acid…
Q: A 1956 dime is made of a silver-copper alloy and has a mass of 2.490 g. The dime was dissolved in…
A: Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…
Q: ered items or incomplete statements is followed by answers or by completions of the statement. ered…
A: Question 27: The Quality coordinating office is the quality control department maintain and store…
Q: Suppose you are titrating an acid of unknown concentration with a standardized base. At the…
A:
Q: Assuming that the uncertainty in the readings does not change, why is it not acceptable to base…
A: Reducing uncertainty in titration is important to determine the desired concentration or the…
Q: A 5.00 mL sample of 0.25 M HBr solution is titrated with 0.35 M NaOH. What volume of NaOH is…
A: We should equal equivalent of both acid and NaOH ion to volume of NaOH Equivalent =…
Q: Sodium hydroxide is a commonly used base in neutralization titrations. It is a normal procedure to…
A: Primary standards are reagents that are used for determining the concentration of the unknown. A…
Q: What mass of FeSO4.(NH4)2SO4. 6H2O is present in a sample if it is titrated to its equivalence point…
A: Given: Volume of KMnO4 = 4.100 mL Concentration of KMnO4 = 0.100 N mass of FeSO4.(NH4)2SO4.…
Q: 19- A sample of limestone is titrated for its value as a neutralizing agent. A sample weighing 1.000…
A: Limestone is CaCO3 Moles of CaCO3 = 1 / 100 = 0.01
Q: Titration of a 25.00 mL sample of acid rain required 12.4 mL of 0.009879 M NaOH to reach the end…
A: Volume of sulphuric acid,V1 = 25.00mL Volume of NaOH,V2 = 12.4mL Concentration of NaOH,M2 =…
Q: The student observed that, addition of Barium chloride solution to an aqueous solutions of samples D…
A: The samples which form a white precipitate with Barium chloride has to be given,
Q: Why are aqueous titrations not suitable for pharmaceutical analysis? use your own words to explain
A: Titration is an analytical method for the quantitative determination of an analyte by adding of…
Q: - A student performed the titration as in this experiment. He transferred a 2.00 mL sample of the…
A:
Q: Titration of a 10.0 mL sample of acid rain required 2.1 mL of 0.0824 M KOH to reach the end point.…
A: Given: Volume of sample is 10 mL. Volume of base is 2.1 mL. Molarity of base solution is 0.0824 M.…
Q: In this experiment you were given the concentration of NaOH(aq). That concentration was determined…
A: Standardization is the process of determining the exact concentration (molarity ) of a solution .…
Q: Titration of a 20.00 mL sample of acid rain required 4.13 mL of 0.08424 M KOH to reach the end…
A: The given reaction is, H2SO4- + 2KOH -----> K2SO4 + 2H2O This means that 2 moles of KOH is…
Q: (i) Give a definition for an acid-base indicator. (ii) List two examples of acid-base indicators…
A: The acidity of a compound can be determined based on the pH of a solution. If the pH of the solution…
Q: The titration of 25.0 mL of an iron(II) solution required 18.0 mL of a 0.115 M solution of…
A: Net ionic equation for the reaction between iron(II) and dichromate is shown below. Number of moles…
Q: It was calculated that 0.00595 moles of acid was added during a titration. If the volume of acid…
A: Molarity is determined as moles of solute per literally of solution. Molarity = molesvolume
Q: The titration of 0.9297 g of KHP (molar mass=204.227 g/mol) requires 41.02 mL of NaOH solution, What…
A: Given: Mass of KHP = 0.9297 g Volume of NaOH = 41.02 mL Molar mass of KHP = 204.227 g/mol
Q: In a titration reaction 20.00 mL of 0.500 M KOH reacts completely with 12.55 mL of sulfuric acid,…
A: Concentration of KOH = 0.500 M Volume of KOH = 20.00 mL (0.02L) Volume of sulfuric acid =…
Q: Through titration with a known standard, we counted that an unknown solution contains 0.048 moles of…
A: Given, Moles of acetic acid = 0.048 mol. The original volume of acetic acid = 120.0 mL. The…
Q: (4) If the end point of the titration was calculated to have occurred at a volume of 17.32 mL and…
A:
Q: A sample containing BTEX What is the appropriate quantitative and qualitative analysis method for it…
A: BTEX i.e Benzene, toulene, ethyl benzene and xylene are volatile organic compounds and are very…
Q: A permanganate solution is prepared by dissolving 20.0123 g KMNO4 in 500 mL of distilled water and…
A:
Q: In the course of various qualitative analysis procedures, the following mixtures are encountered:…
A: It is given that in a qualitative analysis procedure, mixtures are there which contain Ag+ and Mn2+…
Q: In one trial of the standardization of a Na2S2O3 solution, a 10.00 mL volume of 5.00×10-3 M KIO3 is…
A:
Q: What is the titer (expressed in milligrams per milliliters) of a solution of oxalic acid dihydrate…
A:
Q: What is the benefit of using a low concentration of base in titrations?
A: If we use a base having higher concentration then the titration will happen as usual but the result…
Q: True or false: the determination of a molar mass of a compound by the titration method used today…
A: True. The determination of a molar mass of a compound by the titration method used today depends on…
Q: What is the titer(expressed in milligrams per milliliters) of a solution of oxalic acid dihydrate…
A: Given that - Volume of oxalic acid dihydrate Solution = 21.49 mL Mass of calcium oxide = 0.2203 g…
Q: When you mix solutions of lead (II) nitrate and potassium iodide,(i) What is the colour of the…
A: The reaction that takes place when the solution of lead (II) nitrate and potassium iodide mixes is:…
Q: Give a definition for an acid-base indicator. and List two examples of acid-base indicators that you…
A: Acid base indicator are those substance that respond to changes in hydrogen ion concentration . Or…
Q: The chloride ion content of a 250.0-mL seawater sample was titrated against 0.1102 M silver nitrate,…
A: The Chloride ions from the seawater are titrated against silver nitrate and the objective of the…
Q: give a example of a acid-based titration and give a equation
A: An acid is a substance that can release H+ ions in the solution and a base is substance that…
Q: A 0.1824-g sample of an acid is titrated with 0.3090N sodium hydroxide, and 9.256 mL is required to…
A: The solution is given below:
Q: You have identified by titration that a 1.78g sample of bleach contained 90.2mg of NaOCl. What is…
A: Mass percent is the ratio of mass of NaOCl to the mass of sample
Q: Which of the followving refers to the substance being measured in titration?
A: 1. Tirtration is used for the analysis. 2. Here titrant is titrated against standerd solution 3.…
Q: A 25.0mL acetic acid sample was titrated using exactly 69.72 mL of a 0.30M sodium hydroxide solution…
A: Given reaction is- CH3COOH(aq) + NaOH(aq) → CH3COONa(aq) + H2O(l) i.e- 1 mole of CH3COOH reacts…
Q: A student performed a titration on a commercial acid certified to be 0.500 M. Using her data from…
A: The percent error is calculated by the formula, Percentage error=Measured balue-True valueTrue…
Q: In an analysis of vinegar by titration, a student placed the vinegar in the buret and a measured…
A: Please find your solution below : In acidic solutions like vinegar, phenolphthalein is colourless…
Q: give a specific example of gravimetry analysis by enumerating the steps of the analysis
A:
Q: Which of the following is a STRONG base?
A: option: c KOH
Q: Titration of a 25.00 mL sample of acid rain required 13.23 mL of 0.009567 M KOH to reach the end…
A:
Q: In one trial of the standardization of a Na2S2O3 solution, a 10.00 mL volume of 5.00×10-3 M KIO3 is…
A: We have to calculate the Molarity of sodium thiosulfate .
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
- 1.00 grams of table salt was dissolved in 100 mL water and excess AgNO3 reagent was added and yielded 2.3789 grams of precipitate. Calculate the percentage of NaCl in the table salt. Answer must be in 2 significant figures.A 36.0 mL sample of aqueous sulfuric acid was titrated with 0.250 M KOH(aq) until the acid-base indicator signaled that the solution was neutralized. The mixture was then carefully evaporated to dryness, the residue was dried in a drying oven. The residue was then weighed and a value of 861 mg was obtained for its mass. Calculate a value for the volume of the potassium hydroxide solution that was used in the titration from this data. Answer with correct units and significant figures.A 36.0 mL sample of aqueous sulfuric acid was titrated with 0.250 M ROH(aq) until the acid-base indicator signaled that the solution was neutralized. The mixture was then carefully evaporated to dryness, the residue was dried in a drying oven. The residue was then weighed and a value of 861 mg was obtained for its mass. Calculate a value for the volume of the potassium hydroxide solution that was used in the titration from this data. O 12.7 mL O 19.8 mL O48.5 mL 39.5 mL
- A 36.0 mL sample of aqueous sulfuric acid was titrated with 0.250 M KOH(aq) until the acid-base indicator signaled that the solution was neutralized. The mixture was then carefully evaporated to dryness, the residue was dried in a drying oven. The residue was then weighed and a value of 861 mg was obtained for its mass. Calculate a value for the volume of the potassium hydroxide solution that was used in the titration from this data. Answer with correct units and significant figures. Upload Choose a File Next► « Previous Not saved Submit QuizA solution is made by the following steps. 1.) 90.0 mg ± 0.2 mg of dye with molar mass 685.79 g/mol ± 0.02 g/mol is dissolved in a 100.00 mL ± 0.05 mL volumetric flask with water to make solution #1. 2.) 25.00 mL of solution 1 is added 100.00 mL ± 0.05 mL volumetric flask with water to make solution #2. 3.) 25.00 mL of solution 2 is added 100.00 mL ± 0.05 mL volumetric flask with water to make solution #3. Describe how to use the pipettes and the directions above to make the most precise solution #3. Explain why this is the most precise method.please help me The aluminum in a 1.200g sample of impure ammonium aluminum sulfate was precipitatedwith aqueous ammonia as the hydrous Al2O3 · XH2O. The precipitate was filtered and ignitedat 100°C to give anhydrous Al2O3, which weighed 0.2001 g. Express the result of this analysisin terms of % Al.
- Q1) (a) Analyze the effects of contaminants in the gravimetric analysis. (b) A raw sample of NaCl weighing 5.45 g was treated with excess of AgNO3 6.92 g AgCl is obtained. Determine the purity of the NaCl.(c) Discuss the factors which contribute to the formation of precipitateA student was asked to determine the concentration of ammonia, a volatile substance, in a commercially available cloudy ammonia solution used for cleaning. First the student pipetted 25.00 mL of the cloudy ammonia solution into a 250.0 mL conical flask. 50.00 mL of 0.100 mol L-¹ HCl(aq) was immed added to the conical flask which reactedwith the ammonia in solution. The excess (unreacted) HC1 was then titrated with 21.50 mL 0. 050 M Na2CO3 (aq). Calculate the concentration of the ammonia in the cloudy ammonia solution.give a specific example of gravimetry analysis by enumerating the steps of the analysis
- A permanganate solution is prepared by dissolving 20.0123 g KMNO4 in 500 mL of distilled water and boiled for 1 hour to remove any organic material. Following sintered-glass filtration, the solution is quantitatively transferred to a 1.0 L volumetric flask and diluted to volume with distilled water. The permanganate solution was titrated against 0.1023 M oxalic acid prepared in sulfuric acid solution. A 50.00 mL aliquot of oxalic acid solution required 16.68 mL of permanganate solution. A titration blank required 0.04 mL of permanganate. What is the permanganate molarity? 5 H2C204 + 2 MnO4 + 6H* s 10 CO2 + 2 Mn²* + 8 H2OA permanganate solution is prepared by dissolving 20.0123 g KMNO4 in 500 mL of distilled water and boiled for 1 hour to remove any organic material. Following sintered-glass filtration, the solution is quantitatively transferred to a 1.0 L volumetric flask and diluted to volume with distilled water. The permanganate solution was titrated against 0.1023 M oxalic acid prepared in sulfuric acid solution. A 50.00 mL aliquot of oxalic acid solution required 16.68 mL of permanganate solution. A titration blank required 0.04 mL of permanganate. What is the permanganate molarity? 3. 5 H;C204 + 2 MnO¿ + 6H* s 10 CO2 + 2 Mn²* + 8 H2OPhenobarbital was introduced in 1912 for the treatment of epilepsy. It is an anti-convulsant and sedative-hypnotic drug and used to control seizures. The measurement of phenobarbital is by fluorescence method. A 5.00 mL aliquots of an unknown containing phenobarbital were delivered to 50.00 mL volumetric flasks. The following volumes of a standard solution of phenobarbital, 2.00ug/mL, were then introduced to the volumetric flasks before diluting to volume with the corresponding signals on a fluorometer equipment. Find the concentration of phenobarbital in the original unknown sample.
