Ex(1): In the analysis for chloride. The sample weighed (0.8732 gm) and the AgCI (p.p.t) from the sample weighed (1.0292 gm). Calculate the precent of chloride in the sample. At. wt. of Cl= 35.5, Ag = 101.88.
Q: Examine the impact of the following circumstance on the PURITY of the sample. Decide whether the…
A: EDTA is ethylenediaminetetraacetic acid which is an indicator. It has 2 amino and 4 carboxyl groups.…
Q: Make a rough sketch of a titration curve that represents your experimental results. Label the axes:…
A: KHP (potassium acid phthalate) is a weak acid. It has a pH of around 4.0. On the other hand, NaOH is…
Q: В. In her next experiment. she needs to determine the Ksp and identity of a sparingly soluble salt…
A:
Q: 1. A process where impurity is precipitated along with the desired product. 2. Calculate the…
A: Gravimetric analysis is the process in which impurity is also precipitated along with the desired…
Q: В. In his next experiment, he needs to determine the Ksp and identity of a sparingly soluble salt…
A: In the above solution MF2 is sparingly soluble. It is titrated with 0.0110M HNO3.
Q: I need help calculating the remaining values please!!!!
A: A question based on mole concept that is to be accomplished.
Q: The solution may contain one or more of the following cations: Bit3 Mg+2 K+1 Ag+1 Pb+2 Nit2 Hg2+2…
A: What is/are cation present in unknown data sample is given below.
Q: A 0.1093-g sample of impure Na2CO3 was analyzed by the Volhard method. After adding 50.00 mL of…
A:
Q: 5. An accurately measured 2g sample of hydrogen peroxide (H₂O₂-34g/mol) was dissolved in a mixture…
A: Given following balanced Chemical equation - 2KMnO4 + 5H2O2 + 3H2SO4 -----> 2MnSO4 + K2SO4 + 5O2…
Q: Drye quantity of primary standard potassim hydrogen phthalate (CHP) for about 2 heat 110°C (Fig.…
A: Given: mass of KHP = 0.7624 g molar mass of KHP = 204.22 g/mol Titration Initial volume (mL)…
Q: Benzoic acid is not very soluble in water and has a much stronger affinity for organic solvents.…
A: Organic compounds have a greater tendency to soluble in organic solvents and sodium salts have a…
Q: Q2- A 30.0 mL H2C2O4 acidified solution, was treated with 25.0 mL of 0.102 M KMNO4 solution. The…
A:
Q: What was the volume of 6.12 M acetic acid HC2H3O2 needed to prepare the 250 mL acetic acid/acetate…
A: Given that, Volume of buffer solution VB = 250 mL Concentration of acetic acid in buffer solution…
Q: A foot powder sample containing Zn was dissolved on 100.00 mL water and was titrated to the end…
A: The question is based on the concept of complexometric titrations. We have to calculate pZn value.
Q: Part I. Cause and Effect: lIdentify the effect of the condition on the indicated parameter. Write…
A: Higher concentration solution will have more mass of solution. Hence low specific heat. With the use…
Q: 20 aspirin tablets labeled 80mg were dissolved in 100mL of 90% ethanol. A 10mL aliquot was taken and…
A: The acetylsalicylic acid, commonly known as aspirin, is one of the most important analgesic drugs…
Q: A ceric sulfate solution that was standardized using 200 mg of arsenic trioxide (MW 197.84g/n)…
A:
Q: is
A: KD is the distribution coefficient that indicates the amount of sample taken dissolved in the two…
Q: Prove that for a 0.1M NA3PO4 solution the mass balance equation for the H2PO4 - is: [OH=] – [H*] -…
A: IMPORTANT POINTS: Firstly there is an incomplete information provided about the equation to be…
Q: A solution is generated by mixing zinc chloride and sodium hydroxide. The resultant concentrations…
A: Ionic product (KIP) expression for Zn(OH)2 is Zn(OH)2 --> Zn+2 + 2…
Q: Accurately prepare a 50cm stock solution of (approx.) 0.003M potassium permanganate solutic Very…
A: Given that: the volume of potassium permanganate solution = 50 cm3 the volume of potassium…
Q: the following data were the results from six replicate determinations of iron in aqueous samples of…
A:
Q: Given the volume of 0.4810 M NaOH used determine the concentration of 19 ml sample each from…
A: Given that, The concentration of the NaOH is 0.4810 M. The volume of the aqueous layer and the…
Q: The possible reason for the ignition of gravimetric precipitate is I. for its mass to be lower II.…
A:
Q: Gravimetric assay of sulfuric acid involves step of precipitation by: BaCl, Са(ОН)2 AgNO3 FeCl3
A: Thus the correct option is BaCl2
Q: Calculate the gravimetric factor of the following. 2 Fe is sought(Analyte), 1Fe2O3 is weighed…
A: According to the formula, GF =n (FW substance sought)m (FW substance weight)
Q: Calculate the mole fractions of SO2•H2O, HSO3- and SO3 2- in solution at a pH of 3.0, characteristic…
A: Given: pH of 3.0 Total concentration of S(IV) in solution for 20 ppb SO2 in the gas phase.
Q: The weight of 7 ml of vinegar sample was 7.99 g, was required 31.0 ml of 0.3 M sodium hydroxide…
A: Now, the chemical reaction taking place is- CH3COOH + NaOH→CH3COONa + H2O Thus, 1 mole of acetic…
Q: If the Ksp for CaSO, is 2.4x10- calculate the SO2- in CasO. saturated solution.
A: Introduction: We have to calculate the concentration of sulfate ion.
Q: In the standardi zation of HCl using pure anhydrou s sodium carbonate as primary standard for methy…
A:
Q: In gravimetric analysis, co-precipitation occurs alongside with analyte precipitation, resulting in…
A: Distinguish the difference between occlusion andinclusion and compare them using diagrams
Q: Given the following data, prove that the distribution of benzoic acid in water and benzene follow…
A: The total number of moles/mass of benzoic acid is not given to calculate the extracted number of…
Q: A foot powder sample containing Zn was dissolved on 50.00 mL water and was titrated to the end point…
A:
Q: Make an schematic diagram for procedure below: B. %SO3 determination Transfer all precipitate to…
A: We need to make a schematic diagram for the given procedure.
Q: How do you find the delta Hrxn in J/mol?
A: Since you have asked multiple question, we will solve the first question for you. If you want any…
Q: 1- The mercury present in a sample with a mass equal to 0.8142 g was precipitated with an excess of…
A: Given information, Mass sample of mercury = 0.8142 g Mass of product i.e. Hg5(IO6)2 = 0.4114 g
Q: To a 0.5 g sample of impure NaCl are added 0.784 g of pure AgNO3 (MW = 169.88) crystal. This is in…
A: During calculation, it was found that the concentration of KCNS should be 0.028 M. hence solving the…
Q: concentration of 0.10 mg/L. The PAC is added to the stream and the mixture subsequently settled in a…
A: The value of Langmuir constant a and b has to be given,
Q: A foot powder sample containing Zn was dissolved on 200.00 mL water and was titrated to the end…
A:
Q: Calculate the AH° of the borate dissolution at 25°C in kJ mol1, if the 22.12 mL of 0.025 M HCI…
A: Solution- Given data- T= 250C =298K ∆S0 = 61.14 J mol-1 K-1, gas constant = 8.314 J mol-1 K-1
Q: (a) Show that the equation AT, = -k;mB gives MB = -k,wg/ (AT,WA), where wg and wa are the masses of…
A:
Q: 3. The sulfate ion concentration in natural water can be determined by measuring the turbidity that…
A:
Q: Compare the results obtained when soap solution was added to the permanent hard water treated with…
A:
Q: . of T Determination. titriet acid and tedium tydriesxide. of the enthalpy of reaction Molority f…
A: Since you have asked multiple questions, we will solve the first question for you. If you want any…
Q: he sulfate in 266.5 mg sample was precipitated as BaSO4 by addition of 27.00 mL of 0.0340 M BaCl2.…
A:
Q: A 50 mL sample solution containing 8-hydroxyquinoline (MW: 145) was analyzed by adding 25 ml, 0.1 M…
A:
Q: Gravimetric Problems A 516.7-mg sample containing a mixture of K,SO, and (NH,)SO, was dissolved in…
A: Given, Mass of sample: 516.7 mg=516.7×10−3 g BaSO4 yield = 863.5 mg The balanced chemical equation:…
Q: (a) Why is a small amount of MgY2- often added to a water specimen that is to be titrated for…
A:
Q: ort Sheet 20mL in buret ent: 50:50 water:isopropyl alcohol (v/v) 22 °C perature: Volume of pure…
A: Hii there, As there are multiple question posted. we are answering first question. If you need…
Step by step
Solved in 3 steps
- 00 mL of a diprotic acid primary standard solution was accurately prepared to a concentration of 0.1431 M. Three samples of this primary standard solution were used as samples in a titration to standardize an aqueous solution of sodium hydroxide, NaOH, which would be used as a titrant. Using the following table of data for the titration of the primary standard acid with NaOH, calculate the average concentration of NaOH. Trial # Volume of primary standard Initial titrant volume Final titrant volume 1 10.00 mL 8.21 mL 27.22 mL 2 10.00 mL 27.22 mL 46.23 mL 3 10.00 mL 30.28 mL 49.29 mL 0.1506 M 0.0753 M 0.0376 M 0.1431 M 0.0526 MA 50 mL sample solution containing 8-hydroxyquinoline (MW: 145) was analyzed by adding 25 ml, 0.1 M KBrO3, excess KBr and acidified. The mixture was left for 10 minutes in dark place. After this time KI in excess was added followed by titration with 27.9 mL, 0.05 M thiosulfate standard solution. Write balance equations? What is the percent w/v 8-hydroxyquinoline in sample?A sodium thiosulfate solution can be standardized by using it to titrate the iodine liberated by the action of excess KI on a known weight of primary standard K2Cr2O7: Cr2O72- + 6I- + 14H+ → 2 Cr3+ + 3I2 + 7H2O I2 + 2S2O32- → 2I- + S4O62- Calculate the molar concentration of the sodium thiosulfate solution if 31.47 mL of this solution were required to titrate a sample prepared using 0.2177 g pure K2Cr2O7.
- Compare and contrast an anticipatory standard to a reactionary standard by listing and describing some advantages and disadvantages.Calculate the gravimetric factor of the following. 2 Fe is sought(Analyte), 1Fe2O3 is weighed (Precipitate)Make an schematic diagram for procedure below: B. %SO3 determination Transfer all precipitate to the filter paper avoiding any loses during the filtration procedure. One may use a rubber policeman to scrape remaining precipitate in the beaker. Wash the precipitate in the beaker 3x with hot water before transferring to the filter paper. Test the washings with 0.1 M AgNO3 Cloudiness indicates presence of chloride ions; therefore there is a need to wash more the precipitate. Carefully lift the paper out of the funnel, fold it as demonstrated by your instructor and transfer it onto the constant weighed crucible. Dry the crucible cautiously with a small flam, as instructed by your instructor. The flame should be directed at the top of the container, and the lid should be off. Avoid spattering. After drying, char the filter paper by increasing the flame temperature. The crucible should have free access to air. The lid should be kept handy to smother the filter paper in case it catches fire.…
- The student then determined ΔH neutralization for the reaction of sodium hydroxide and acetic acid, using the procedure described in this module. The student added 100.0 mL of 0.8500M NaOH to 100.0 mL of 0.8404M acetic acid. Prior to and following the mixing of the acid and base solutions, the following temperature-time data were collected. g) Identify the limiting reagent and briefly explain why it is limiting. h) Find ΔH neutralization for the reaction.Hexanoic acid was added to an immiscible biphasic solvent sysem, water and CCl4 at 20.0OC and the equilibrium concentrations of hexanoic acid were determined to be 3.66 g/L in H2O and 67.0 g/L in CCl4. Caluclate the distrubution coeffiecent (D1) of hexanoic acid in CCl4 with respect to water.A pH probe/meter uses the following equations: Ecell = L + 0.0592 log a1 = L - 0.0592 pH Where L = L1 + EAg/AgCI + Easy= constants L1 = - 0.0592 log a2 a1 = activity of analyte solution a2 = activity of internal solution Questions: How will measured pH value be affected vs “real” pH if the temperature of the sample is 30C when pH was measured? How will measured pH value be affected vs “real” pH if HCl in pH electrode, became 0.15M instead of 0.1M? How pH value will be affected vs “real” pH if the glass of the pH electrode is not fully hydrated? Please answer all questions and provide a brief explanation
- -Please determine the ksp for Cu(OH)2. pH for solution was 5.25 Show ice box for chemical equation. please show all steps to solution clearlyIn gravimetric analysis, co-precipitation occurs alongside with analyte precipitation,resulting in the introduction of impurity and excess mass. Occlusion and inclusion areamong the sources of impurities. Distinguish the difference between occlusion andinclusion and compare them using diagramsSources of Error Determine the relationship between the observed/apparent value (EX) VERSUS that of the true value (ET) for the quantity being sought by writing either <, >, or = on the space provided. TOPIC: Measured mass of the precipitate 1. Overignition which causes the conversion of BaSO4 precipitate to BaO. EX _____ ET2. Precipitate was not washed thoroughly. Ex _____ ET TOPIC: Standardization of Titrant 3.Distilled water was not equilibrated to room temperature before the preparation of NaOH titrant. EX _______ ET