Q: 2. Find the pH of a 0.500M solution of NH4OH with a Kb= 1.75 X 10-5. ANSWER: pH=
A: The term pH is the negative logarithm of the concentration of hydrogen ions [H+]. The term pOH is…
Q: 5. Using the values of AS°, and AH, calculate AG for each of the following reactions. a. Pb(s) +…
A:
Q: Which of the following is a primary standard for NaOH? A. None of these B. Potassium acid phthalate…
A: The major problem while weighing sodium hydroxide is that the solid absorbs moisture from its…
Q: Calculate the pH of a 2.0M propanoic acid solution (HC 3 H 5 O 2 , Ka = 1.3 x 10 -5 ). Show all work…
A: In this question, we want to determine the pH of the Solution. How we can determine, you can see…
Q: you think? Write in “BULLET POINTS”. An alkaline solution was prepared with LiOH in such a way that…
A: Here are some limitations of modern periodic table: 1. There is no proper place for hydrogen in the…
Q: will H3N titrate with 1.0M Ba(OH)2?
A: For any titration to be possible, one components needs to be acid and the other needs to be the base…
Q: The zinc contained in a 0.7555-g sample of foot powder was titrated with 21.27 mL 0.01645 M EDTA.…
A:
Q: 5.) Regarding the second preliminary test, if 100.0 ml of 0.050 M BaCl, is combined with 150.0 mL of…
A: In order to calculate Q we have to find concentration of Ba2+ and CO32-
Q: omework ubmitted Aug 8 at 11:15pm 1/1 pts Question 13 The [OH ] and the pH of 0.035 M KOH at 25 °C…
A:
Q: Calculate the weight of solid Ba(OH)2 (MW = 171.34g) in order to make a 0.39 litre of the base…
A: Here we are required to mass of Ba(OH)2.
Q: 8. (a) Compare between Electron ionization (EI) and Chemical ionization methods.
A:
Q: In 100-200 words, Differentiate acidimetry from alkalimetry.
A: We have to differentiate acidimetry from alkalimetry as follows in step 2:
Q: Suppose that you use 0.75 g of iron in this experiment. What is the minimum volume of 1.5 M CuSO4…
A: Given following balanced Chemical equations - a) using eq. (5-1) - Fe(s) + Cu2+(aq) -> Fe2+(aq)…
Q: E OC 25 50 75 100 125 150 175 Volume of 0.100 M NaOH (ag) (mL) the major species present at point A?…
A: In the titration, KOH is added dropwise to H3PO4 solution. So , At A point, only H3PO4 is…
Q: 2. Chloride in a brine solution NaCI (FM: 58.44) could be determined by the Volhard method. A…
A: The concentration of brine solution is determined as follows. NaCl=MAgNO3×VAgNO3-MKSCN×VKSCNVNaCl…
Q: pka E
A:
Q: Determine the Ksp for each solution. Cu(OH)2 Ba(OH)2 Mg(OH)2
A:
Q: 7. For aldehydes, a common quantification method is: A) Polarimetry B) Iodometry (back titration)…
A: Aldehyde is represented as - R - CHO, where R = Alkyl group In presence of an oxidising agent,…
Q: Acidic Basic Neutral Answer Bank H] = 1.0 x 10 pl = 3.46 pOH = 5.41 OH =26 x 10 %3D %3D pOH = 8.31…
A:
Q: Calculate the ionic strength of 0.00025 M La(IO3)3 (assuming complete dissociation at this low…
A: Explanation Ionic strength Ionic strength denotes to a measure of the concentration of ions…
Q: 6. Find the pH of a 1.00-L aqueous solution prepared with 14.23 g of tris (FM 121.00) plus 5.67 g of…
A:
Q: 9. If only 0.9% of 0.50 M solution of a weak base was ionized. Calculate its Kb value? * 1.6 x 104…
A:
Q: Find [H] and the pH of 0.05 M LiNO3.
A: pH is used to determine the concentration of hydronium ion.
Q: Find the pH of 0.15 M HClO and 0.25 M NaClO. Ka of acid at 25 C is 3.98 x 10^-8
A: Given data The concentration of HClO, [HClO] = 0.15 M The concentration of NaClO, [NaClO] = 0.25 M…
Q: What is the pH of a solution that is 0.28 M in acetic acid, HC2H3O2, and 0.69 M in sodium acetate,…
A:
Q: 31-40. B, ACID: CONJUGATE BASE: USING ICE TABLE HA(acid), H (hydronium ion), A (conjugate base) HA…
A: 4.HA → H+ + A-Kc = [ H+][A-][HA]x2(0.65 - x)= 7.1×10-4 value of x is small and neglect itx =…
Q: If the base (NaOH) is standardized to 0.12 M in Part A of this experiment, calculate the amount of…
A: The reaction between oxalic acid dihydrate and NaOH is ; H2C2O4·2H2O + 2NaOH → Na2C2O4 + 4H2O From…
Q: The pH of a liquid is 8.2 + 0.1. Find [H1] and its absolute and relative uncertainty.
A:
Q: 3. Calculate the pH of a 0.250 M solution of NH4A. (Some useful informatiíon is given below.) Ka for…
A: PH is defined as the negative logarithm of H+ concentration for the salt of weak acid and weak base…
Q: 2. Chloride in a brine solution NaCI (FM: 58.44) could be determined by the Volhard method. A…
A:
Q: If 5 mL of 20% w/v aqueous solution of furosemide is diluted to 10mL, what will be its final…
A: Given that: Volume of solution = 5 mL Strength of solution = 20% w/v Volume added = 10 mL Final…
Q: What is the ionic strength of 0.50 M Al2(SO4)3 + 0.10 M Na2SO4?
A: A chemical compound consists of two or more different elements which are bonded with each other…
Q: 2. Chloride in a brine solution NaCI (FM: 58.44) could be determined by the Volhard method. A…
A: Answer : Option a. 2.877 g/L Given : Molarity of AgNO3 = 0.1182 M Volume of…
Q: Calculate the pH at 25 °C of a 0.46 M solution of potassium butanoate (KC,H,CO,). Note that butanoic…
A: Since HC3H7CO2 is a weak acid with pKa = 4.82 Hence the pKb of its conjugate base i.e C3H7CO2- = 14…
Q: Predict the pH(>7,<7,=7) of the following solution: NaBr, K2SO3, NH4NO2, Cr(NO3)3
A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…
Q: Pre-lab question #10-2: The PH of a 0.1 M MCI (M† is an unknown cation) was found to be 4.7.…
A: Hydrolysis is the interaction of anion or cation of the salt with water to produce an acidic or…
Q: The value of Ka for acetic acid is 1.75 X 1025. Find Kb for acetate ion.
A: Given information, Ka for acetic acid is 1.75 X 1025
Q: 5-30. Generate a curve for the titration of 50.00 mL of a solution in which the analytical…
A:
Q: 7. If the solution with the pH of 1.30 had a concentration of 0.05M, what is the percent ionized for…
A: pH of a solution is defined as the negative logarithm of hydronium ion concentration.Given pH of the…
Q: e solution is 25 °C.) und your answer to 3 signifi
A:
Q: please help with this quantitative analysis question!!
A: The concentration of H+ in the solution can be calculated as follows:
Q: Consider a weak acid, HA, for which Ka = 7.1x10-4. Calculate [H*] in a solution that is 0.45 M in…
A:
Q: Calculate the value of [N 21 eg if [H 2] eq = 1.5 M, [NH 3) eq 0.5 M, and Kc = 2. N 2(8) + 3 H 2(8)…
A: Kc is the ratio of the equilibrium concentrations of product over equilibrium concentrations of…
Q: What is the pH of the initial 30.0 mL strong acid analyte HZ sample if upon titrated with 15.0 mL…
A:
Q: 2a. EDTA titration of Ca²+ + Mg2+ ions at pH 10 using calmagite indicator Data Trial Trial 2 Volume…
A: In the above experiment, Ca2+ and Mg2+ ion concentration in tap water and in bottle water…
Q: The pH of a 4.0 × 10-3 mol dm-3 solution of weak base is 10.4. Calculate the Kb of the weak base.
A: A base is a chemical compound which takes a proton. Base which is not dissociated completely in a…
Q: Find the conditional formation constant for Sr(EDTA)2- at pH 11.00, where log Kf is 8.72 and ayt- is…
A:
Q: 2- a. Find the conditional formation constant for Mg(EDTA)² at pH 9.00. b. Find the concentration of…
A:
Q: 10 ml, 25 ml, 50 ml and 60 ml of titrant containing 0.1 M Ce4 + on 50 mL of analyte containing 0.1 M…
A: Solution Balanced equation; Ce⁴+ + Fe2+ --------->Ce3+ +Fe3+ E0 (Fe3+/Fe2+) =0.68V E0(Ce4+/Ce3+)…
Q: Q4. A 5.00 mL aqueous sample containing hydrogen peroxide was diluted to 25 mL and analyzed by…
A: From the balanced redox reaction in the acidic medium, concentration of hydrogen peroxide in the…
What is [H+] with uncertainty for a solution of pH 7.5 ± 0.2?
Thank you!
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
- A pH meter can measure the concentration of H+ with an uncertainty of 5% between pH 4 and pH 8. What is the uncertainty in pH at pH = 6.00?mix 500 ml of 0.1 M HCl solution with 300 ml of 2 M Ba (OH) 2 solution a) indicate the environment of the solution after mixing b) What color will the detectors, phenophthalein and litmus get?What is the maximum metallic concentration in 100.0 liters of water from a metallic hydroxide with a Ksp = 3.99 x 10-20 at pH 3.0, 7.0, and 10.0? Show all work and report final answers with three significant figures.
- Calculate the ionic strength of 0.00025 M La(IO3)3 (assuming complete dissociation at this low concentration and no hydrolysis reaction to make LaOH2+). (with correct sig figs)15.0 grams of an unknown acid is dissolved to a final volume of 100.0 ml and measured to have a pH of 2.4. If Ka=5.0x10-5, what is the MW of the Acid?The voltage measured by the pH meter is linearly proportional to the "H+ concentration" of the analyte solution. True or false? Is H+ concentration correct?