Q2.4of the following statemets which one is FALSE aboutindicators?a) somemoreindicators can be used for titrationsthan onedistinct pH range.b) An indicator isone10-foldexcess of itsacidicdifferent colour when there is abasic form.colourd) An indicatar couldc) The indicator must change colour at the equivalencepoint of a titrationaverwhen there is aform, anda10-fold excess of itsbe the weak acidbase component of a buffer.ar weals

Indicators are substances that change colour when they are added to acidic or alkaline solutions.…

Q2.4 of the following indicators? following statemets which one is FALSE about a) some indicators can be used for titrations over distinct pH range. more than one b) An indicator is one colour when excess of its 10-fold acidic different colour when there is a basic form. d) An indicator could there is a c) The indicator must change colour at the equivalence point of a titration. form, and a 10-fold excess of its base component of a buffer be the weak acid ueals

Q2.4 of the following indicators? following statemets which one is FALSE about a) some indicators can be used for titrations over distinct pH range. more than one b) An indicator is one colour when excess of its 10-fold acidic different colour when there is a basic form. d) An indicator could there is a c) The indicator must change colour at the equivalence point of a titration. form, and a 10-fold excess of its base component of a buffer be the weak acid ueals

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Which indicator could be used to titrate aqueous NH3 with HCI solution? Acid Color- Indicator Range Change Color pH (a) pink 1.2-2.8 (b) blue 3.4 - 4.6 (c) yellow 6.5 - 7.8 (d) colorless 8.3 -9.9 (e) none of these O B O C O < O U E
A Total-ionic strength adjustment buffer with an acidic pH is needed to make a NaF stock solution to determine the concentration of F- of the standard solutions. Explain the importance of maintaining the pH and ionic strength of the buffer solution.
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A buffer is made up of equal volumes (451.8 mL of each) of 0.812 M A H and 0.885 M A minus. 24.51 mL of 0.712 M HCl is added to the buffer. How many moles of A H are present after the addition of HCl? Please use correct significant figures. Answer: (0.384) (mol)
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Would a 0.010M buffer solution or a 0.10 M buffer solution have a greaterbuffering capacity for neutralizing the addition of an acid or a base? Explain.
Pls help ASAP ON ALL ASKED QUESTIONS PLS PLS
#19.16
Example: - How many grams ammonium chloride and how many millilitres 3.0M sodium hydroxide should be added to 200ML water and diluted to 500mL to prepare a buffer of pH9.50 with salt concentrated of 0.10M?
Ule the Keferences to access important values if needed for this yestinn When a 23.2 mL sample of a 0.386 M aqueous hypochlorous acid solution is titrated with a 0.438 M aqueous bariem hydroside solution. (1) What is the pH at the midpoint in the titration? (2) What is the pH at the equivalence point of the titration? (3) What is the pH after 15.3 ml. of barium hydroxide have been added? Submit Answer 2 question attempts remainng