1.0 M NaOH is used as a pH standard in Table 8.1. Use the equations in the introduction to the lab to calculate the concentration of hydronium ions, hydroxide ions and the pH and pOH of the base solution respectively. O1.0 M; 1.0 x 10-14 M: 14.00; 0.00 O1.0 x 10-14 M; 1.0 M; 14. 00; 0.00 O1.0 M; 0.010 x 10-14 M; 14.00; 0. 00 O0.010 x 104 M: 1.0 M: 14.00; 0.00
Q: A 0.128 g sample of KHP (HKC8H4O4) required 28.54 mL of NaOH solution to reach a phenolphthalein…
A: Solution:- Given data = 0.128 g of KHP (HKC8H404) Volume of NaOH used = 28.54 mL = 0.02854 L Molar…
Q: uch 36.5 g 1 mol of HCI = 36.5 g/mol Examples: Calculate the number of moles in 200 mg of CaO? in 10…
A:
Q: What is the net ionic equation for a solution with BaCl2 and addition of HC2H3O2 and K2CrO4? What is…
A: We can determine the net ionic equation for a reaction from the balanced chemical equation. We need…
Q: Complete and balance in standard form NaOH+H2SO4
A: When sodium hydroxide reacts with sulfuric acid it produces sodium sulfate (salt) and water. This…
Q: An unknown volume of 2.50 M H2SO, was diluted to 50 ml using water. The diluted solution was…
A: Introduction: We have to calculate volume of sulphuric acid.
Q: 1000 μl of 1M NaCl stock solution (aq). How you would perform serial dilution to obtain 10-1,…
A: in laboratory, a standard solution is prepared which is called as stock solution.the other solution…
Q: Materials/Chemicals: Volumetric flasks Acid-base indicators: Bromophenol Blue Bromocresol green…
A: For preparation of buffer solution, require chemical and their properties is given table below.
Q: 1. Calculate the H30* and OH concentrations according to the given ph values. Solution pH [H3O] [OH]…
A: We can fill this table by using below mentioned formulas. pH=-log [H3O+] [H3O+] = 10−pH, pH + p OH…
Q: When the following equation is balanced properly under acidic conditions, what are the coefficients…
A: Given reaction is HNO3+H2C2O4 → NO+CO2
Q: An equation which list individually all of the ions present as either reactants or products in a…
A: Step 1: Hello. Since the question contains multiple subparts, the first three subparts are solved.…
Q: When the following equation is balanced properly under basic conditions, what are the coefficients…
A: Since you have asked multiple question, we will solve the first question for you. If you want any…
Q: pH and pOH of [OH–] = 2.51×10-9 M
A: Relation between OH- and pOH is as follows: pOH= -logOH- and pH and pOH is as follows: pH + pOH = 14…
Q: Ammonia (NH3) is a colorless gas with a pungent smell and is quite soluble in water. The Henry's Law…
A: Henry's law relates the pressure of a particular gas present above the solvent and solubility of…
Q: When the following equation is balanced properly under acidic conditions, what are the coefficients…
A: Here we are required to balance the redox reaction
Q: Which statement is NOT correct? pH meter should always be standardized before using to…
A: For the accurate measurement of pH, the pH-meter must be standardised by a buffer solution of known…
Q: <Ch09_Acids and Bases Strength of Electrolytes Reset Help weak electrolyte A 20 mL solution…
A: The species which gets completely dissociated into its constituent ions are termed as Strong…
Q: A 0.9550 g sample of ASA was dissolved in 40.1 mL of standard NaOH. The excess NaOH was neutralized…
A: Since you have posted a question with multiple sub-parts, we will solve first three subparts for…
Q: If the concentration of fluoride anion and aluminum cation was increased to 5 M, by how much would…
A: The reduction potential if Al3+ is negative and that of F2 is positive. This means Al will undergo…
Q: What is the pH of the solution after mixing 0.171 g of Mg(OH), (MW=58.321 g/mol) with 18 mL of…
A: We have to calculate the pH of resulting solution.
Q: For an acid and base reaction, select ALL statements that are TRUE. Supporting information: You can…
A: As per Q&A guidelines of portal I solve first question because it comes under multiple question…
Q: Typical "hard" water contains about 80.2 mg of Ca2* per liter. Calculate the maximum concentration…
A:
Q: Calculate the pH and pOH of 0.30 M HNO3 solution. Kw= 1.0 x 10-14
A: Given data: Concentration of HNO3 solution = 0.30 M, Kw = 1.0×10-14. Nitric acid (HNO3) is the…
Q: How do I find the 2 Precipitation reactions and the 2 Color change reactions?
A: A chemical reaction is symbolic representation of the conversion of substances to new substances.
Q: Determine the concentration of 7.13 g zinc nitrate (MW = 189.4 g/mol) dissolved in 200.0 mL…
A: Given, Weight of zinc nitrate = 7.13 g Molecular weight (MW) of zinc nitrate = 189.4 g/mol Volume of…
Q: Oxidation-reduction reactionsa. can be synthesis or decomposition reactions.b. have one reactant…
A: Redox reactions – The transfer of electrons between any two species resulting in simultaneous…
Q: Calculate the number of equivalents of antacid per gram of tablet. Determine the cost per equivalent…
A: The number of moles of antacid neutralized by HCl is calculated as the difference in the total…
Q: 1. Calculate the H30* and OH concentrations according to the given ph values. Solution pH [H,O']…
A: pH is a scale is a logarithmic scale used to specify the acidity or basicity of an aqueous solution.…
Q: 21 (aq) + S,0, (aq) (ag) nhta
A: In physical chemistry, chemical kinetics is studied for the understanding of the rate of a chemical…
Q: 0.1 M NH4CI solution, using the given pH data, calculate value of (Ka or Kb) 1.0 x 10-9 O 1.0 x 10-6…
A: Since NH4Cl is a salt of weak base and strong acid so we can use hydrolysis formula for this salt
Q: Weighed quantity of dry potassium bromide 1,5560 gr (M=167,000 g/mol) dissolved in water with…
A: Measuring the quantity of a solution of a known concentration of titrant that is needed to react…
Q: Calculate the pH of a solution that has an [OH-] = 4.40 x the 10-3
A:
Q: 8 g of potassium chloride is dissolved in a quart of distilled water. Calculate the pH value of the…
A: Here 8 gram of KOH is dissolved in a quart of distilled water. We have to calculate the pH of…
Q: Calculations for Acetate Buffer Solutions Molarity of acetic in acetate buffer (below is…
A: Molarity = Moles of soluteL of solution Moles = Molarity x L of solution
Q: NaOHbom 0.001 het place in waste viase bon ringe ef and refill with de noitoloa bion oilaxo lo…
A: Given, Molarity of H3PO4 = 0.481M. Volume of Ba(OH)2 = 24.7mL. Molarity of Ba(OH)2 = 0.695M. The…
Q: When the following equation is balanced properly under acidic conditions, what are the coefficients…
A: For balancing the equation in acidic medium when have to find the oxidation and reduction reaction.…
Q: - balanced equation for the following reaction oc aq) + HNO2 (aq) → I3 (aq) + NO (aq) HNOL 31 -> 2No…
A: Redox reaction, I-(aq.) + HNO2(aq.) ---> I3-(aq.) + NO(aq.) Step -1 : splitting into half…
Q: 1. State Whether following statements are true (T) or False (F) in the space provided. a) Electron…
A: a) True b) True c) True d) False e) True
Q: QUESTION NO. 1: A 0.097 N silver nitrate solution of 56.3 ml was used to titrate two samples of…
A: Solution stoichiometry is mainly based on the calculation of moles and volumes. These two values are…
Q: Phosphate buffered saline (PBS) is buffered to a pH of 7.40, the pH of human blood, with the H₂PO4…
A: Given: pH=7.40Ka=6.31×10-8
Q: Calculate the molarity of 150.0 mL of sodium hydroxide solution needed to react with 65.7 mL of a…
A: Please note- As per our company guidelines we are supposed to answer only one question. Kindly…
Q: 2H,0(1) = H30+(ag) + OH (aq) Kw - 1.0 x 10-14 at 25 °C Kw=5.5x 1014 at 50°C Based on this data,…
A: Ordered state to less ordered state is the change in phase of the system. This change is called…
Q: A Complete and balance the reaction: HCI (aq) + H20 () --> ? B. Consider a 3.22x10 5 M HCI (aq)…
A:
Q: What is the pH of the solution after mixing 0.114 g of Mg(OH), (MW=58.321 g/mol) with 16.5 mL of…
A: We have to predict the pH of resulting solution.
Q: When the following equation is balanced properly under acidic conditions, what are the coefficients…
A: Steps to balance the equation - Separate half cell reactions. Given reaction doesn't have acidic or…
Q: /cvg.cengagenow.com/ilm/takeAssignment/takeCovalentActivity.do?locator=Dassignment-take&takeAssignme…
A: Determine number of moles of each reactant: 1 mL = 0.001 L
Q: Calculate AH for the reaction CH4 (g) + NH3 (g) → HCN (g) + 3 H2 (B), Bi
A: Given reactions are 1. N2 (g) + 3 H2 (g) --> 2 NH3 (g) ∆H = -91.8 KJ 2. C(s) + 2 H2 (g)…
Q: Selenous acid is a diprotic acid, for Ka1 = 9.43 x 10-3 and Ka2 = 7.39 x10^-8. Determine the…
A:
Step by step
Solved in 2 steps with 2 images
- The first step in purifying the urine collected on the ISS is to treat every liter of urine with 20 mL of 1.0 M H2SO4. To simplify the calculations, lets assume that urine is water. a) What is the pH of a solution of 20. mL of 1.0 M H2SO4 added to 1.00 L water? To determine this, you can safely assume that 100% of the H2SO4 reacts to form H3O+ and HSO4- ions. Use pKa2 (1.92) to determine if any more protons are added to the solution from HSO4-.One strategy for dealing with the acidification of lakes is periodically to add powered limestone (CaCO3) to them, resulting in pH of 10.95. Calculate the Ca2+ concentration in the lake. CO2 in atmosphere 370 ppm KH,CO2 = 0.033 mol/(L∙atm) Ka1 = 10-6.3 Ka2 = 10-10.3 Ksp,CaCO3 = 4.57 x 10-9For the determination of basic species in 0.1878 g Talcid sample; 20 mL of 0.1009 M HCl solution was added to the sample and the necessary procedures were carried out and titrated with 0.1097 M NaOH solution. Since 10.2 mL of base solution is consumed at the end of the titration, which of the following is the% base amount in CaCO3? (CaCO3: 100,087 g / mol) A. 23.96B. 55.1C. 45.1D. 42.1
- Determine the pH of a solution prepared by dissolving 0.35 mole of ammonia chloride in 1.0l of 0.25M aqueous ammonia.kb for ammonia equals 1.77×10^-5Calculate the pH of a solution that is prepared by dissolving 0.23 mol of hydrofluoric acid (HF) and 0.57 mol of hypochlorous acid (HClO) in water and diluting to 3.60 L. Also, calculate the equilibrium concentrations of HF, F-,HClO, and ClO2. (Hint: The pH will be determined by the stronger acid of this pair.)Chemists have defined the pH (Hydrogen Potential) of a solution by pH = -log[H+] where [H+] represents the concentration of the hydrogen ion in moles per liter. The pH scale ranges from 0 to 14 depending on a solution’s acidity or alkalinity. Values below 7 indicate progressively greater acidity, while above 7 are progressively more alkaline. Normal, unpolluted rain has pH of about 5.6. Since the pH scale is logarithmic, keep in mind that there is tenfold in hydrogen ion concentration for each pH unit. An environmental concern involves the destructive effects of acid rainfall ever had a pH of 2.4, what is the hydrogen ion concentration? A. 0.004 mole per liter B. 0.002 mole per liter C. 0.39 mole per liter D. 0.25 mole per liter
- During the titration of an HClO4 solution with 0.10320 M NaOH, a student, Lovely became distracted and overshot the endpoint. A fellow student Ashley suggested that he should record the present volume of NaOH added and titrate the excess with a standard acid solution. If the original sample volume was 25.000 mL, the volume of NaOH added was 28.060 mL. It took 3.4700 mL of 0.10940 M HCl to back-titrate the NaOH and calculate the molar concentration of the original HClO4Express the concentration of acetic acid in both samples as % by mass of acetic per 100mL of solution given : %= mass/ volumex100% Given: NaOH vs CH3COOH Burette solution is NaOH and the pipette solution is 5.0 mL of Vinegar Titration Initial burette reading Final burette reading Volume of NaOH consumed Average volume of NaOH Approximate 0.0 mL 20.1 mL 20.1 mL 20.3 mL Titration 1 0.0 mL 20.9 mL 20.9 mL Titration 2 0.0 mL 20.0 mL 20.0 mL To find the average volume Average volume = 20.1 mL + 20.9 mL + 20.0 mL320.1 mL + 20.9 mL + 20.0 mL3 = 20.3 mL Concentration of Vinegar = Volume of NaOH * Concentration of NaOHVolume of vinegarVolume of NaOH * Concentration of NaOHVolume of vinegar = 20.3 mL * 0.0647 M5.0 mL20.3 mL * 0.0647 M5.0 mL = 0.2627 M Concentration of NaOH = Volume of H2SO4 * Concentration of H2SO4Volume of NaOHVolume of H2SO4 * Concentration of…5.What are the limitations of modern periodic table you think? Write in “BULLET POINTS”. An alkaline solution was prepared with LiOH in such a way that 0.65 g dry LiOH was directly mixed with 0.6 M 650 mL LiOH solution and finally 350 mL more water was added to it. Find the final pH of the solution. You need to consider 100% dissociation of LiOH. [Ref: 7Li, 1H, 16O]
- Lareina the laboratory technician is given the task of making a solution containing HOBr (Ka=2.8×10−9) and KOBr and testing its behavior when strong acid or base is added to it. Part 1 First, Lareina combines 86.1 g KOBr and 250 mL of 1.45 M HOBr, and adds enough distilled water to make 800 mL of solution. What is the pH of this solution? pH solution = Part 2 Next, Lareina adds 12.0 mL of 2.20 M HNO3 to 360 mL of the solution made in Part 1. What is the pH of the solution after the HNO3 is added? pH after HNO3 added = Part 3 Finally, Lareina adds 10.0 mL of 2.20 M NaOH into 365 mL of the solution made in Part 1. What is the pH of the solution after the NaOH is added? pH after NaOH added =Lareina the laboratory technician is given the task of making a solution containing HOBr (Ka=2.8×10−9) and KOBr and testing its behavior when strong acid or base is added to it. Part 1 First, Lareina combines 86.1 g KOBr and 250 mL of 1.45 M HOBr, and adds enough distilled water to make 800 mL of solution. What is the pH of this solution? pH solution = Part 2 Next, Lareina adds 12.0 mL of 2.20 M HNO3 to 360 mL of the solution made in Part 1. What is the pH of the solution after the HNO3 is added? pH after HNO3 added = Part 3 Finally, Lareina adds 10.0 mL of 2.20 M NaOH ito 365 mL of the solution made in Part 1. What is the pH of the solution after the NaOH is added? pH after NaOH added =Students Mola and Rity were tasked to analyze the acidity of a 10.0-mL fermented milk sample diluted with water in a 250-mL volumetric flask. Mola obtained a 15.0-mL aliquot of this solution, diluted it to 50.0 mL, and then titrated this diluted sample. Titration data were given to Rity and she found out that the 50.0-mL diluted sample contains 0.21 mmol of lactic acid. MW: Lactic Acid (90.08) a. What is the lactic acid concentration (in M) of the titrated sample? b. Determine the lactic acid content (in M) of the 10.0-mL fermented milk sample. c. What is the lactic acid concentration (in %w/v) of the 10.0-mL fermented milk sample?